chemistry terms 4 midterm
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| what is the si unit for mass? | kilogram
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| what is the si unit for length? | meter
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| what is the si unit for volume? | liter
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| what is the si unit for temperature? | kelvin
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| what is the si unit for time? | second
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| mega (m) | ten to the sixth power
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| kilo (k) | ten to the third power
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| deci (d) | ten to the negative first power
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| centi (c) | ten to the negative second power
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| milli (m) | ten to the negative third power
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| micro | ten to the negative sixth power
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| nano (n) | ten to the negative ninth power
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| what is volume? | amount of a 3 dimensional space
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| what is the basic si unit for volume? | meter cube
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| 1 dm3 | 1 liter
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| 1l | 1,000 ml
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| 1ml | 1 cm3
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| meter is what according to volume? | volume of a cube
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| what is temperature? | average kinetic energy of atomic motion
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| what does the speed of kinetic movement give us? | the sense of wheither something is hot or cold
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| fahrenheit (f) | equal to 5/9 a celsius or kelvin degree
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| clesius (c) | bassed off freezing and boiling points of water
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| What is the same degree as a kelvin degree? | a celsius degree
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| Kelvin (k) | basic si unit for temperaturebased on the value of absolute zero
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| what happens at absolute zero? | molecular motion stops
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| absolute zero is what degrees kelvin? | zero
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| absolute zero is what degrees celsius? | -273
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| absolute zero is what degrees fahrenheit? | -460
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| freezing point is what degrees kelvin? | 273
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| freezing point is what degrees celsius? | 0
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| freezing point is what degrees fahrenheit? | 32
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| boiling point is what degrees kelvin? | 373
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| boiling point is what degrees celsius? | 100
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| boiling point is what degrees fahrenheit? | 212
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| how do you convert celsius to kelvin? | add 213 to the celsius
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| how do you convert fahrenheit to celsius? | subtract the fahrenheit degree by 21 then divide that number by 1.80
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| what is density? | amount of matter in given volume of substance
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| how do you calculate density? | divide the mass by the volume
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| how do you calculate volume? | divide the mass by the density
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| how do you calculate mass? | multiply density by volume
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| what is volume displacement? | solid matches volume of water once the solid is placed in water
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| what is matter? | has mass and occupies space
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| solid | is rigid, has a fixed shape and a fixed volume
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| liquid | has a definite volume, takes the shape of the container
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| gas | doesn't have a fixed shape or volumetake the shape and volume of the container
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| plasma | super heated gas
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| solid to a liquid is? | melting, heat energy is gained
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| liquid to a gas is? | evaporation, heat energy is gained
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| solid to a gas is? | sublimation, heat energy is gained
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| gas to a liquid is? | condensation, heat energy is lost
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| liquid to solid is? | freezing, heat energy is lost
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| gas to a solid is? | deposition, heat energy is lost
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| gas to a plasma is? | ionization
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| what is an atom? | smallest unit of an element that has all the properties of that element
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| what is an element? | substance that cannot be broken down into other substances by a chemical process
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| what is a compound? | substance composed of given combination of elements that can be broken down into those elements by chemical means
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| what type of change is a compound into an element? | chemical change
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| Do compounds have different elements? | yes, always
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| Compounds _____________ have same composition even though they have different atoms | always
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| What does all matter consist of? | mixtures of pure substances
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| what is a mixture? | a mixture has a variable composition
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| what is a pure substance? | always has the same composition throughout (whether compound or element)
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| what can mixtures always be seperated into? | pure substances (element or compound)
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| a mixture has | two or more substances
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| homogenous mixture | same composition throughout solution
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| what are examples of homogenous mixtures? | salt water, air, brass
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| heterogeneous mixture | mixture whose regions have different properties form those in other regions
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| what is an example of a heterogeneous mixture? | a salad
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| what may a mixture be classified as? | solution, suspension, or colloid
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| What has an effect on the properties of matter? | the size of the particles in a mixture
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| solution is what type of mixture? | homogeneous
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| solution | particles are too small to settle out of solution, they are trapped by a filter
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| what is an example of a solution? | sugar water
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| suspension is what type of mixture? | heterogenous mixture
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| suspension | particles who settle out of mixture or are trapped by a filter, these particles are larger than the particles in a solution
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| what is an example of a suspension? | chocolate milk
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| colloid | bettwen small particles in a solution and the large particles in a suspension
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| Do colloid particles seperate into layers? | no
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| what is an example of a colloid? | fog
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| Can you use a filter to seperate particles? | no
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| what is energy? | the ability to do work
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| what is temperature | measurement of molecular motion and the energy of a substance
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| what is heat? | the flow of energy due to a temperature
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| what is one way to change energy? | change the temperature of a substance
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| temperature and heat | are not the same thing
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| heat is | energy
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| temperature is | man-made, arbitrary scale showing direction of heat flow
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| heat enters | rising of temperature
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| heat leaves | declining of temperature
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| what is heat measured by? | calorimeter
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| What is temperature measured by? | therometer
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| What is heat measured in? | joules
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| what is temperature measured in? | degrees
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| heat transfer | molecules never mix, yet energy transformed from "hotter" water to "colder" water
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| what is the heat transfer equation? | add the initial hot temperature to the initial cold temperature and then divide by two
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| exothermic reaction | when a reaction releases heat or energy
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| what is an example of an exothermic reaction? | a match
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| endothermic reaction | when a reaction absorbs energy or heat
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| what is an example of an endothermic reaction? | melting ice
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| calorie (cal) | the amount of energy (heat) required to raise the temperature of one gram of water by one celsius degree
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| 1 calorie is what in joules? | 4.184 joules
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| what is specific heat capacity? | amount of energy required to change the temperature of one gram of a substance by one celsius degree
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| specific heat formula | multiply specific heat of substance by mass of substance by temperature change
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| isotope | atoms with the same number of protons but different number of neutrons
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| what do all atoms of the same element have? | same number of protons and same number of electrons
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| what equals a zero net charge | when the protons and neutrons balance out
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| what did the dalton theory assume? | all atoms of an element are identical
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| what did james chadwick discover? | atomic nuclei contains neutrons
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| Dalton's changed theory | all atoms of the same element contain same number of protons and electrons, but atoms of a given element may have different number of neutrons
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| what is the reason for isotopes? | the discovery of the neutron
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| atomic number | number of protons in the nucleus
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| atomic mass | sum of the number of neutrons plus the number of protons in a given nucleus
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| isotope notation | specify which isotope of element your talking about
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| what did dimitri mendeleev first create? | the periodic table of elements used
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| how did dimitri mendeleev organize the elements? | by their atomic weight
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| periodic table | chart grouping elements by specific properties
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| what does the periodic table help predict? | some properties of the elements compared to each other
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| atom size decreases when | you move from left to right across the periodic table
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| atom size increases when | you move down a column in the periodic table
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| energy required to remove an electron increases when | you move left to right on the periodic table
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| energy required to remove an electron decreases when | you move down a column in the periodic table
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| ability to form a chemical bond increases when | you move left to right on the periodic table
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| ability to form a chemical bond decreases when | you move down a column in the periodic table
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| how are elements on the periodic table arranged? | by periods (rows) and groups (columns)
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| atomic increases when | you move across a row or period on the periodic table
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| what do columns of elements on the periodic table define? | the element groups
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| how are elements classified? | by their properties
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| 3 main categories of elements | metals, nonmetals, metalloids
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| most metals share what | common properties
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| some properties of metals are | lustrous (shiny) malleable (may be hammered) are good conductors of heat and electricity
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| what are most elements? | metals
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| what are the three groups of metals? | alkali metals, alkaline earth metals, and transition metals
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| what are the two transition metal groups? | lanthanides and actinides
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| where are alkali metlas located on the periodic table? | group 1A this does not include hydrogen
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| what is a form of alkali metals | salt and other compounds
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| alkali metals are | less dense than other metals
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| alkali metals have | the largest atom size of elements in their row
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| what type of ionic charge do alkali metals have? | a plus one charge
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| are alkali metals highly reactive? | yes
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| where are alkaline earth metals located on the periodic table? | group 2A
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| alkali earth metals form | many compounds
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| what type of ionic charge do alkaline earth metals have? | a plus two charge
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| alkali earth metals are smaller in size than what? | alkali metals
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| transition metals are located where on the periodic table? | on groups 3-12 (1B-8B)
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| metals are | very hard
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| metals have | high melting and boiling points
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| transition metals are | conductors and malleable
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| what do transition metals form? | positively charged ions
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| transition metals include | most elements
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| where are lanthanides located on the periodic table? | top row of the top row section
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| lanthanides are. | silvery metals that tarnish easily
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| lanthanides are relatively | "soft"
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| lanthanides have high | melting and boiling points
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| lanthanides may react to form.... | many different compounds
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| where are actinides located on the periodic table? | bottom row bottom section placed below the periodic table
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| actinides are all what? | readioactive
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| what do actinides form? | positively charged ions
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| actinides are | reactive metals that commonly form compounds with nonmetals
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| metalloids are what? | elements having properties of both metals and nonmetals
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| what varies in metalloids? | boiling points, melting points and densities
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| metalloids are excellent | semiconductors
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| nonmetals are | elements that do not have properties of metals
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| nonmetals are poor | conductors
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| where are nonmetals located on the periodic table? | groups 3A-8A including hydrogen
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| where are nonmetals found on the periodic table? | top right side of periodic table, seperated by a diagonal line
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| where are halogens found on the periodic table? | group 7A
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| are halogens metals or nonmetals? | they are nonmetals
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| what type of ions do halogens form? | ions with a negative one charge
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| halogens are very | reactive
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| where are noble gases found on the periodic table? | group 8A
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| are noble gases metals or nonmetals? | they are nonmetals
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| noble gases do not | react
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| what is the law of definite proportions? | a given compound contains the same elements in exactly the same proportions by mass, regardless of size or sameple
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| what is the law of conservation of mass? | the mass of the products of a reaction equals the mass of the reactants
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| what is the law of multiple proportions? | the mass ratio for one of the elements in a compound that combines with a fixed mass of another element can be expressed in small whole numbers
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| what does the law of multiple proportions apply to? | different compounds formed from the same two elements
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| what is atomic mass measured in? | atomic mass unit (amu)
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| atomic mass is the average mass of what | isotops
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| mole | SI unit for the amount of a substance
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| how do you express moles as a quantity of mass | molar mass
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| one mol of any element has what? | a mass in grams
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| What is Bohr's model? | 1911 constructed a model of hydrogen atoms with quantized energy levels
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| quantizied energy is a | specific amount of energy
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| What did Bohr's model suggest? | electrons could jump to different orbits by absorbing or emitting a photon of light with exactly the correct energy content
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| What did Bohr's model energy states represent? | certain allowed circular orbits
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| What did Bohr's model only work for? | hydrogen
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| Who developed the wave mechanical model? | Broglie and Schrodigner
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| What did the wave mechanical model show? | electrons may act as a particle and a wave
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| What did the wave mechanical model work for? | every element
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| What did Bohr's model assume? | electrons move in circular orbits, electrons described as orbitals
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| What may Bohr's model tell us? | proability of finding an electron a certain distance from the nucleus
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| What can't Bohr's model tell us? | when electrons occupied a point or how it moves in the atom
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| how does an electron spin? | on its axis
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| How is an electrons spin represented? | by an up or down arrow
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| electrons have | equal but opposite spins
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| How many electrons may each orbital have | two : opposite spin
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| What is the Pauli Exclusion Principle? | orbital may hold a maximum of 2 electrons, those 2 electrons must have opposite spins
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| How is the number of electrons in an orbital represented? | by a superscript
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| What is the Aufbau Principle? | electrons in the atom will occupy the lowest available orbital
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| Energy levels may | overlap
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| What may the wavelength of a wave tell us? | the frequency of a wave
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| How are wavelengths expresed? | meters or nanometers
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| What is the frequency of a wave dependent on? | the wavelength
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| When wavelength increases | frequency decreases
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| When wavelength decreases | frequency increases
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| What is the "c" factor? | the speed of light
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| What does the dual nature of matter state? | matter can act as a particle and a wave
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| Who determined a way to actually calculate the energy of photons? | plank
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| How do you calculate a change in energy? | multiply plank's constant by the frequency
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| How did Albert Einstein say electromagnetic radiation may be viewed? | a stream of particles called photons
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| What does energy emitted in the form of photons correspond to? | the charge in energy of the excited atoms
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| Different wavelengths carry different what | different amount of energy per photons
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| what are the five trends that may be found on the periodic table? | atomic radius, electron affinity, electronegativity, ionization energy, ionic size
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| What is the atomic radius? | the measured distance between the nuclei of two identical atoms chemically bonded together
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| How is the atomic radius defined? | by the edge of last energy level
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| What is the trend for atomic radius on the periodic table? | gradual decrease in size from left to right
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| What is ionization energy? | energy needed to recieve one of an atom's electrons
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| Ionization energy is a measure of | how strongly an atom holds onto its outermost electrons
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| electron affinity | measure of an ability of an atom to attract or gain an electron
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| What type of charge do atoms have when they tend to accept an electron? | a negative charge
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| Electron affinity does not have | noble gases
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| In electron affinity the closer to the full outer shell, what? | the higher the affinity, more energy
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| What is the trend for electron affinity? | increases from left to right and from down to up
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| Electronegativity | reflects the ability of an atom to attract electrons in a chemical bond
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| What is the most electronegative element? | Flourine
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| What does electronegativity correlate to? | an atoms ionization energy and electron affinity
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| What is the trend for boiling and melting point? | increase as move left to right and down to up
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| electromagnetic radiation | energy traveling through space containing radiation
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| what does wavelength tell us? | about the frequency
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| what is frequency measured in? | hertz (hz)
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| qualitive measurement | something is unique and is not always in numerical form
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| A qualitive measurement may be | observable
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| quantitive measurement | something that is expressed in numerical form, using numbers
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| accuracy | the results are in the range that they should be in but aren't spot on
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| precision | being spot-on or there
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| true or false: the celsius degree is smaller than the Fahrenheit unit | false
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| In calculations where significant figures are involved, our final answer has | the lowest number of sig figs in our data
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| what does the f orbital contain | both actinides and lanthanides
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| d orbital | contains a total of 10 electrons
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| halogens | very reactive
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| p orbital | first found in second principle energy level
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| metalloids | have properties of both metals and nonmetals
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| noble gases | elements of this group don't want to react with other elements
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| s orbital | only contains 1 orbital
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| non-metals | poor conductors, compromises the right hand side of the periodic table
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| what is the density formula? | mass divided volume
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| does size effect density? | no
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| how do you name type 1 binary ionic compounds? | cation doesn't change, add -ide to the anion
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| hwo do you name type 2 binary ionic compounds? | same rules as type one, but you add roman numerals because they are transition metals
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| how do you name type 3 binary ionic compounds? | use the name of the first element and add -ide to the anion, use prefixes
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| how do you name an acid if it has oxygen in the anion? | if it ends in ate add icif it ends in ite add ous
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| how do you name an acid if it doesn't have oxygen in the anion? | add hydro and ic to the anion
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| What are the different types of waves? | gamma rays, x-rays, ultraviolet rays, infrared rays, radar, fm, tv, shortwave, am
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| all elements on the periodic table form what | molecules
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| what is a molecule | a collection of atoms that behave as a unit with no electrical charge
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| molecules and compounds are | different
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| Why are most elements reactive? | their atoms want to combine with other elements and form compounds
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| diatomic molecules | are made up of two atoms
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| neutral atoms | atoms with no net charge
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| how is a cation produced? | when one or more electrons are lost from its neutral atom
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| how is a anion produced? | when one or more electrons are gained from its neutral atom
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| what must the net charge of any compound be? | zero
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