Chemistry Final Exam

Front 1

Anything that occupies space and has mass

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matter

Front 2

a form of matter that has a definite (constant) composition and distinct properties

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substance

Front 3

a combination of two or more substances in which the substances retain their distinct identities

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mixture

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a mixture in which the composition is the same throughout

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homogeneous mixture

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a mixture in which the composition is not uniform

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heterogeneous mixture

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a substance that cannot be separated into simpler substances by chemical means

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element

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a substance composed of two atoms or more elements chemically united in fixed proportions

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compound

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a property that can be measured and observed without changing the composition or identity of a substance

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physical property

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a property that can only be observed if you carry out a chemical change to it

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chemical property

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quantity of matter in a given sample of a substance

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matter

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length cubed

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volume

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mass of an object divided by its volume

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density

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the force that gravity exerts on an object

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weight

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what is length measure in

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meter (m)

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what is mass measured in

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kilogram (kg)

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what is time measured in

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second (s)

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what is temperature measured in

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kelvin (K)

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what is the amount of a substance measured in

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mole (mol)

Front 19

what is tera(T)-

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10^12

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what is giga(G) -

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10^9

Front 21

what is mega(M) -

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10^6

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what is kilo(k)-

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10^3

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what is deci(d) -

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10^-1

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what is centi(c)

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10^-2

Front 25

what is mili(m)

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10^-3

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what is micro(u)

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10^-6

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what is nano(n)

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10^-9

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what is pico(p)

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10^-12

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the SI base unit of temperature

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kelvini

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how do you convert Celsius to Kelvin

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add 273

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how do you convert Fahrenheit to Celsius

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(F-32) * 5/9

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how do you convert Celsius to Fahrenheit

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9/5 * (C + 32

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Who formulated a precise definition of the invisible building blocks of matter that we call atoms

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John Dalton

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Name the hypothesis on the atomic theory

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1. elements are composed of extremely small particles
2. all atoms of a given element are identical.
3. Compounds are composed of atoms of more than one element.
4. A chemical reaction involves only the separation, combination, or rearrangement of atoms.

Front 35

state this law:
different samples of the same compound always contain its constituent elements in the same proportion by mass. who made this law

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law of definite proportions
John Proust

Front 36

state this law:
if two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers

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law of multiple proportions

Front 37

state this law and who made it:

matter can neither be created nor destroyed

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law of conservation of matter
John Dalton

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what is the basic unit of an element

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atom

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the emission and transmission of energy through space in the form of waves

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radiation

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negatively charges particles

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electrons

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dense central core within the atom

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nucleus

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positively charged particles

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protons

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neutral particles having a mass slightly greater than that of protons

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neutrons

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the number of protons in the nucleus of each atom of an element

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atomic number (Z)

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the total number of neutrons and protons present in the nucleus of an atom of an element

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mass number (A)

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atoms that have the same atomic number but different mass numbers

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isotopes

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where are the alkali metals

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Group 1A

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Where are the alkaline earth metals

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Group 2A

Front 49

Where are the halogens

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Group 7A

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Where are the noble gases

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Group 8A

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an aggregate of at least two atoms in a definite arrangement held together by chemical forces (chemical bonds)

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molecule

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an ion with a net positive charger

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cation

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an anion with a net negative charge

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anion

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formed from cations and anions

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ionic compound

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express the composition of molecules and ionic compounds in terms of chemicial symbols

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chemical formulas

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shows the exact number of atoms of each element in the smallest unit of a substance

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molecular formula

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shows which elements are present and the simplest whole-number ratio of their atoms

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empirical formula

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mono-

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1

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di-

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2

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tri-

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3

Front 61

tetra-

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4

Front 62

penta-

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5

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hexa-

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6

Front 64

hepta-

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7

Front 65

octa-

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8

Front 66

nona-

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9

Front 67

deca-

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10

Front 68

a substance that yields hydrogen ions (H+) when dissolved in water

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acid

Front 69

mass equal to one-twelfth the mass of one carbon-12 atom.

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atomic mass unit

Front 70

what is avogadro's number

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6.0221367 * 10^23

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the amount of substance that contains as many elementary entities (atoms, molecules, particles) as there are atoms in exactly 12g of the carbon-12 isotope

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mole

Front 72

the mass of 1 mole of units

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molar mass (M)

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the sum of the atomic masses in the molecule

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molecular mass

Front 74

what is percent composition by mass

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percent by mass of each element in a compound

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a process in which a substance is changed into one or more new substances

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chemical reaction

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starting materials in a chemical reaction

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reactants

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the substance formed as a result of a chemical reaction

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products

Front 78

the quantitative study of reactants and products in a chemical reaction

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stoichiometry

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the reactant used up first in a reaction

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limiting reagent

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reactants present in a quantities greater than necessary to react with the quantity of the limiting reagent

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excess reagents

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the amount of product that would result if all the limiting reagent reacted

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theoretical yield

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the amount of product actually obtained from a reaction

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actual yield

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actual yield/theoretical yield x 100%

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percent yield

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a homogeneous mixture of two or more substances

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solution

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the substance present in a smaller amount

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solute

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the substance present in a larger amount

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solvent

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the solute initially is a liquid or a solid and the solvent is water

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aqueous solution

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a substance that, when dissolved in water, results in a solution that can conduct electricity

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electrolyte

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does not conduct electricity when dissolved in water

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nonelectrolyte

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formation of an insoluble product

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precipitation

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an insoluble solid that separates from the solution

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precipitate

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the maximum amount of the solute that will dissolve in a given quantity solvent at a specific temperature

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solubility

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a reaction that involves the exchange of parts between the two compounds

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metathesis reactions

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proton donor

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Bronsted acid

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proton acceptor

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Bronsted base

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reaction between an acid and a base

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neutralization reaction

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electron-transfer reactions

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oxidation or redox reactions

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half-reaction that involves loss of electrons

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oxidation reaction

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half-reaction that involves the gain of electrons

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reduction reaction

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donates electrons

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reducing agent

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accepts electrons

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oxidizing agent

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the number of charges the atom would have in a molecule if electrons were transferred completely

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oxidation number

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a reaction in which two or more substances combine to form a single product

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combination reaction

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the breakdown of a compound into two or more components

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decomposition reaction

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a reaction in which a substance reacts with oxygen, usually with the release of heat and light to produce a flame

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combustion reaction

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an ion or atom in a compound is replaced by an ion of another element

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displacement reaction

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amount of solute present in a given quantity of solven or solution

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concentration of solution

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number of moles of solute per liter of solution

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molarity

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a solution of accurately known concentration

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titration

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added gradually to another solution of unknown concentration until the chemical reaction is complete

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standard solution

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instrument for measuring atmospheric pressure

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barometer

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law that states the fixed amount of gas at a constant temperature is inversely proportional to the volume of the gas

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Boyle's law

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law that states that the volume of a fixed amount of gas maintained at constant pressure is directly proportional to the absolute temperature of the gas

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Charles's law

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law that states that at constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of the gas present

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Avogadro's law

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law that states that the total pressures of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone

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Dalton's law of partial pressures

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the gradual mixing of molecules of one gas with molecules of another by virtue of their kinetic properties

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diffusion

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law that states under the same conditions of temperature and pressure, rates of diffusion for gases are inversely proportional to the square roots of their molar masses

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Graham's law of diffusion

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the process by which a gas under pressure escapes from one compartment of a container to another by a small opening

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effusion

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the capacity to do work

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energy

Front 120

the study of heat change in chemical reactions

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thermochemistry

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any process that gives off heat

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exothermic

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any process that retains heat

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endothermic

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law that states that energy can be converted from one form to another, but cannot be created nor destroyed

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first law of thermodynamics

Front 124

the distance between identical points on successive waves

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wavelength

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number of waves that pass through a particular point in 1 second

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frquency

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the vertical distance from the midline of a wave to peak of trough

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amplitude

Front 127

what scientist calculated the mass of an electron

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Milliken

Front 128

Who said that atoms and molecules emit or absorb energy only in specific amounts called quanta

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Planck

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light emission only at specific wavelengths

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line spectra

Front 130

describes the distribution of electrons in hydrogen and other atoms

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quantum numbers

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states as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to the atomic orbitals

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Aufbau principle

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one-half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule

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atomic radius