Chemistry
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The scientific system of writing numbers | scientific notation
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Give the scientific Notation of 1,000,000,000 | 10^9
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Give the scientific notation of' 1,000,000 | 10^6
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Give the scientific notation of 1,000 | 10^3
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Give the scientific notation of 100 | 10^2
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Give the scientific notation of 1 | 10^0
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Give the scientific notation of 0.01 | 10^-2
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Give the scientific notation of 0.000001 | 10^-6
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Give the scientific notation of 0.000000001 | 10^-9
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method to measure weight, length, and volume | metric system
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simple, logical, and efficient measurement system | metric system
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basic units of measurements of the metric system | grams, liters, and meters
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Basic measurement of weight | grams (g)
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Basic measure of weight | liter (L)
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Basic measure of distance | meter (m)
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Tera- abbreviation means? numerically | T-
10^12
1 quadrillion times
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Giga- abbreviation? means? numerically? | G-
10^9
1 billion times
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Mega- abbreviation? means? numerically | M-
10^6
1 million times
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kilo- abbreviation? means? numerically? | k-
10^3
1 thousand times
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hecto- abbreviation? means? nummerically? | h-
10^2
1 hundred times
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deka- abbreviation? means? numerically? | D-
10^1 times
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deci- abbreviation? means? numerically? | d-
10^-1
1 tenth of
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centi- abbreviation? means? numerically? | c-
10^-2
1 hundredth of
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milli- abbreviation? means? numerically? | m-
10^-3
1 thousandth of
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micro- abbreviation? means? numerically? | u(backwards)
10^-6
1 millionth of
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nano- abbreviation? means? numerically? | n-
10^-9
1 billionth of
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pico- abbreviation? means? numerically? | p-
10^-12
1 trillionth of
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femto- abbreviation? means? numerically? | f-
10^-15
1 quadrillionth of
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3 most common temperature systems | Fahrenheit, Celsius, nad Kelvin
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temperature measuring system used only in the United States, its territories,Belize, and Jamaica. | Fahrenheit
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Rarely used for any scientific measurements except body temperature. | Fahrenheit
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Zero degrees is the freezing point of sea water or heavy brine at sea level. | Fahrenheit
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32 degrees is the freezing point of pure water at sea level. | Fahrenheit
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212 degrees is the boiling point of pure water at sea level. | Fahrenheit
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Most people have a body temperature of 98.6 degrees | Fahrenheit
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temperature system used in the rest of the world and by the scientific community. | Celsius/Centigrade
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zero degrees is the freezing point of pure water at sea level. | Celsius
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100 degrees is the boiling point of pure water a sea level. | Celsius
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Most people have a body temperature of 37 degrees | Celsius
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Used only in the scientific community | Kelvin
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zero degrees is -273 degrees Celsius and is thought to be the lowest temperature achievable or absolute zero | Kelvin
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The freezing point of water is 273 | Kelvin
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The boiling point of water is 373 | Kelvin
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Basic building block of all molecules | Atom
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Atom's physical structure | Nucleus
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At the center of the atom and is composed of protons and neutrons | Nucleus
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When are atoms most stable? | When an orbital is full
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positive electrical charge | protons
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negative charge | electrons
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no charge | neutrons
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an atom that is electrically charged | ion
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an atom that has a positive charge | cation
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an atom that has a negative charge | anion
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defined by its properties | matter
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rows of the periodic table | periods
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columns of the periodic table | groups
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energy required to remove the outermost electron from the atom. | ionization energy
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ability to attract electrons | electronegativity
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what location is the alkali metals in the periodic table? What are the properties? | Group 1
metals with one outermost electron. form 1+ ions
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what location are the alkaline earth metals in the periodic table? what are the properties? | Group 2
metals with two outermost electrons. Form 2+ ions
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where are the transition metals located in the periodic table? | Groups 3-10
Metals that usually form colored ions and solutions. Have multiple oxidation states.
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Where are the Halogens located in the periodic table? | Group 17
Nonmetals with seven outermost electrons.
Form 1- ions
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Where are the noble gases located in the periodic table? | Group 18
Nonmetal gases that do not react because they have full outermost PELs
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Two important numbers or properties of atoms that can be obtained from the periodic table are? | atomic number & mass
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number of protons in the nucleus, and it defines an atom of a particular element. | atomic number
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what is the atomic mass of an atom? | average mass of each of that element's isotopes.
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different kinds of the same atom that vary in weight | Isotopes
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What is it called when a an element or atom exists in combination with other elements? | compound
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How is an equation written> | Reactants ----> Products
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In any chemical reaction, an arrow between the reactants and the products is drawn out. What does the arrow symbolize? | the direction of the reaction
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what does the law of conservation of mass state? | Mass cannot be created or destroyed during a chemical reaction. Therefore, once the reactants have been written and the products predicted, the equation must be balanced.
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A state in which reactants are forming products at the same rate that products are forming reactants. | Equilibrium
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Name 4 ways to increase the reaction rate | increase the temperature in the reaction, increase the surface area of the reactants, add a catalyst, or increase the concentrations of reactants.
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If you increase the temperature in the reaction what happens? | causes the particles to have a greater kinetic energy causing them to move faster. Contact is when the chemical reactions will occur.
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What happens when you increase the surface area of the particles in the reaction? | Gives the particles more opportunity to come into contact with one another.
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accelerates a reaction by reducing the activation energy or the amount of energy necessary for a reaction to occur. | catalyst
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what happens when you increase the concentration of the reactants? | It will cause more chance collisions between the reactants and produce more products.
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Homogeneous mixture of two or more substances | solution
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can be a liquid in a liquid, a solid in a liquid, or a solid in a solid. | solutions
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name the four types of solutions | compounds, alloys, amalgams, emulsions
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Mixtures of different elements to create a single matter | compound
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solid solutions of metals to make a new one such as bronze, which is copper and tin, or steel, which is iron and carbon, tungsten, chromium, and manganese | alloys
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a specific type of alloy in which another metal is dissolved in mercury | amalgams
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mixtures of matter that readily separate such as water and oil. | emulsions
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How is percent concentration expressed? | weight/weight; grams/grams
weight/volume; grams/liters
volume/volume; milliliters/liter
**mg/100mL
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How is Molar concentration expressed? | a mole=6.02x10^23
mol/L
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Name the five main types of chemical reactions | synthesis
decomposition
combustion
single replacement
double replacement
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two elements combine to form a product. 2K(+) + 2Cl(-) ---> 2KCL | Synthesis
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opposite of synthesis because it is the breaking of a compound into its component parts. | NaCl ---> Na(+) + Cl(-)
decoposition
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self-sustaining, exothermic chemical reaction usually initiated by heat acting on oxygen and a fuel compound such as hydrocarbon. | combustion
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replacement reactions involve ionic compounds; consist of a more active metal reacting with an ionic compound containing a less active metal to produce a new compound | single replacement
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joining of one atom | chemical bonding
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electrostatic attraction between two oppositely charged ions, or a cation and an anion. | ionic bond
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generally formed between a metal and a nonmetal | ionic
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formed when two atoms share electrons, generally in pairs, one from each atom. | covalent bond
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in a covalently bonded compound, if the electrons in the bond are shared equally, then the bond is termed ____. | nonpolar
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___ is based on the difference in eletronegativity values for the elements involved in the bond. | polarity
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NOT BONDING INTERACTIONS; Weaker forces of attraction between whole mlecules | intermolecular forces
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attraction for a hydrogen atom by a highly electronegative element. | hydrogen bond
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attraction of one dipole on one molecule for the dipole of another molecule | dipole-dipole interactions
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how is a dipole created? | when an electron pair is shared unequally in a covalent bond between two atoms or elements
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