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