question

scientific method

answer

a logical, systematic approach to the solution of a scientific problem

question

steps of the scientific method

answer

1. Define the problem 2. Research the problem 3. Form a hypothesis 4. Perform an experiment (Test hypothesis) 5. Analyze data 6. Communicate results

question

independent variable

answer

variable that is manipulated

question

dependent variable

answer

the factor that is being measured or controlled during the experiment

question

scientific theory

answer

a hypothesis that is supported by experimental evidence over a long period of time

question

scientific law

answer

a concise statement that summarizes the results of many observations and experiments

question

extensive properties

answer

a property that depends on the amount of matter

question

mass

answer

the amount of matter that an object contains

question

volume

answer

the amount of space occupied by an object

question

solid

answer

a form of matter that has a definite shape and volume

question

liquid

answer

a form of matter that has a definite volume, but not a definite shape

question

gas

answer

a form of matter that does not have a definite shape or volume

question

physical change

answer

a process where some properties of a material change, but the composition of the material stays the same

question

reversible

answer

usually when matter changes states such as from a solid to a liquid the change can be reversed

question

irreversible

answer

usually when matter changes so that it cannot be reversed, ex: cutting or cracking an egg

question

mixture

answer

a physical blend of two or more components

question

heterogeneous mixture

answer

a mixture that is not uniform in composition, ex: chicken noodle soup

question

homogeneous mixture

answer

a mixture in which the composition is uniform (also called a solution), ex: vinegar, oil

question

filtration

answer

a process that separates a solid from a liquid in a heterogeneous mixture, ex: colander separating water from pasta

question

distillation

answer

boiling liquid to produce a vapor then condensing the liquid to separate a homogeneous mixture, ex: removing salt from salt water

question

element

answer

the simplest form of matter that has a unique set of properties

question

compound

answer

a substance that contains two or more elements chemically combined in a fixed proportion

question

chemical change

answer

a change that produces matter with a different composition than the original matter

question

chemical property

answer

the ability of a substance to undergo a specific chemical change

question

chemical reaction

answer

a process that involves the rearrangement of the molecular or ionic structure of a substance as opposed to a change in a physical form or a nuclear reaction

question

ways to recognize chemical changes

answer

1. Transfer of energy 2. A change in color 3. The production of a gas 4. The formation of a precipitate

question

precipitate

answer

a solid that forms and settles out of a liquid mixture

question

Law of Conservation of Mass

answer

states that in any physical change or chemical reaction mass is conserved, mass is neither created nor destroyed

question

During any chemical reaction the mass of the products is ALWAYS equal to the mass of the reactants.

answer

true

question

measurement

answer

is a quantity that has both a number and a unit, a fundamental process to the experimental sciences

question

scientific notation

answer

a given number is written as the product of two numbers: a coefficient and a 10 raised to a power, ex: 602,000,000,000,000,000,000,000 = 6.02 x 10^23

question

accepted value

answer

the correct value based on reliable references

question

experimental value

answer

the value measured in the lab

question

error

answer

the difference between the accepted value and the experimental value , error = experimental value - accepted value

question

percent error

answer

the absolute value of the error divided by the accepted value, multiplied by 100%, percent error = error/accepted value x 100%

question

significant figures

answer

all of the digits that are known, plus the last digit that is estimated

question

rules for significant figures

answer

1. Every non zero digit is considered significant, ex: 1,2,3 2. Zeroes occurring between non zero digits are significant, ex: 101 = 3 significant digits 3. Leftmost zeroes occurring to the left of non zero digits are NOT significant, ex: 0.0021 has 2 significant digits 4. Zeroes at the end of a number and RIGHT of a decimal point are significant, ex: 43.00 has 4 significant figures 5. Zeroes at the rightmost end of a measurement that lie to the LEFT of a decimal point are not significant, ex: 7000 has one significant figure

question

International System of Units (SI)

answer

a revised version of the metric system, adopted by the international community in 1960

question

most common units used by chemists

answer

1. Meter(m)- length 2. Kilogram(kg)- mass 3. Kelvin(K)- temperature 4. Second(s)- time 5. Mole(mol)- amount of substance 6. Liter(L)- volume of a substance 7. Joule(J)- unit of energy

question

commonly used prefixes

answer

Mega(M)- 1 million times larger Deci(d)- 10 times smaller Kilo(k)- 1000 times larger Centi(c)- 100 times smaller Hecto(h)- 100 times larger Milli(m)- 1000 times smaller Deka(da)- 10 times larger Micro - 1 mil times smaller

question

weight

answer

a force that measures the pull on on a given mass by gravity

question

common metric units of volume

answer

liter, milliliter, cubic centimeter (cm3) and microliter, one cubic centimeter = 1 milliliter

question

Celsius scale

answer

sets the freezing temperature of water at 0 and boiling temperature at 100, Celsius = Kelvin - 273

question

Kelvin scale

answer

does NOT use degrees and sets 0 at absolute zero which is equal to -273.15 Celsius, Kelvin = Celsius + 273

question

energy

answer

the capacity to do work or to produce heat, measured in joule (J), 1 joule = 0.2390 cal

question

calorie

answer

the quantity of heat that raises the temperature of 1 g of pure water by 1 degree Celsius, 1 calorie = 4.184 J

question

conversion factor

answer

a ratio of equivalent measurements ex. 100cm/1m or 1m/100cm

question

dimensional analysis

answer

is a way to analyze and solve problems using the units, or dimension, of the measurements

question

density

answer

ratio of the mass of an object to its volume, density= mass/volume

question

atom

answer

the smallest particle of an element that retains its identity in a chemical reaction

question

Democritus

answer

believed that atoms were indivisible and indestructible

question

Dalton's Atomic Theory

answer

1. States all elements are composed of tiny indivisible particles called atoms 2. Atoms of the same element are identical. Atoms from one element are different from atoms from another element 3. Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds 4. Chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction

question

subatomic particles

answer

atoms can be broken down into smaller objects, which are called subatomic particles

question

three types of subatomic particles

answer

proton, neutron, electron

question

Cathode Ray Experiment

answer

In 1897 J.J Thompson passed electric currents through gasses at low pressure. He sealed gas in a tube and used oppositely charged electrodes that produced a glowing beam that traveled from one end to the other. This led to the discovery of the electron

question

Rutherford's Gold Foil Experiment

answer

1911; Fired alpha particles (Helium atoms without electrons) into a sheet of gold foil, most of the alpha particles went straight through, some deflected at large angles, led to the discovery of the nucleus

question

relative atomic mass

answer

? since the actual mass of an atom is so small we use relative atomic mass which is seen on the periodic table ? since hydrogen is the smallest atom (having a mass of 8.275 x 10^-25) we say that hydrogen has a relative atomic mass of 1 ? example: carbon has a mass 12 times larger than hydrogen, therefore, it has a relative mass of 12

question

atomic mass

answer

? Atomic mass is based on a Carbon-12 isotope. ? An atomic mass unit (amu) is used to describe the mass of an atom ? An atomic mass unit (amu) is defined as one twelfth of the mass of a carbon-12 atom.

question

neutron

answer

subatomic particles with no charge that are located in the nucleus of an atom, discovered by Chadwick in 1932

question

Thompson's Theory

answer

Thompson's theory that subatomic particles were evenly distributed throughout the nucleus of an atom, later proven to be inncorrect

question

proton

answer

positively charged subatomic particles, that are located in the nucleus of an atom, discovered by Goldstein in 1886

question

atomic model

answer

states that the nucleus is the central core of an atom and is composed of protons and neutrons. The electrons are distributed around the nucleus and occupy almost all of the volume of an atom, improved the plum pudding model but was still incomplete

question

isotope

answer

atoms that have the same number of protons but a different number of neutrons, since isotopes will have a differing number of neutrons, their mass will be different as well

question

periodic table of elements

answer

an arrangement of elements in which the elements are separated into groups based on a set of repeating properties ? each horizontal row is called a period ? each vertical row is called a group or family

question

Dalton's Model

answer

John Dalton proposed that all matter is composed of very small things which he called atoms. This was not a completely new concept as the ancient Greeks (notably Democritus) had proposed that all matter is composed of small, indivisible (cannot be divided) objects. When Dalton proposed his model, electrons and the nucleus were unknown.

question

Thompson's "Plum Pudding" Model

answer

The electron was discovered by J.J. Thomson in 1897. However, the atomic nucleus had not been discovered yet and so the "plum pudding model" was put forward in 1904. In this model, the atom is made up of negative electrons that float in a "soup" of positive charge. However, even with the Plum Pudding Model, there was still no understanding of how these electrons in the atom were arranged.

question

Rutherford's Model

answer

His new model described the atom as a tiny, dense, positively charged core called a nucleus surrounded by lighter, negatively charged electrons. A simplified picture of this is shown alongside. This model is sometimes known as the planetary model of the atom.

question

Bohr's Model

answer

There were, however, some problems with Rutherford's model: for example it could not explain the very interesting observation that atoms only emit light at certain wavelengths or frequencies. Niels Bohr solved this problem by proposing that the electrons could only orbit the nucleus in certain special orbits at different energy levels around the nucleus.

question

James Chadwick

answer

James Chadwick discovered the neutron in 1932.

question

Quantum Mechanical Model

answer

The Quantum Mechanical Model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus.

question

atomic orbitals

answer

? a region of space in which there is a high ? ? ? probability of finding an electron ? each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found ? three sublevels: s,d,p,f S- spherical P- dumbbell shaped D- cloverleaf shaped F- more complicated "D" orbital

question

electron configuration

answer

the way in which electrons are arranged into various orbitals around the nuclei of atoms

question

rules to find electron configuration (there are exceptions)

answer

1. Aufbau Principle 2. Pauli Exclusion Principle 3. Hund's Rule

question

Aufbau Principle

answer

electrons occupy the orbitals of lowest energy first

question

Pauli Exclusion Principle

answer

an atomic orbital may contain at most two electrons (must have opposite spins)

question

Hund's Rule

answer

states that each orbital must have at least one electron with the same spin before being able to move on to the next orbital

question

amplitude

answer

the height of a wave

question

wavelength

answer

the distance between the crests (peaks)

question

frequency

answer

the number of wave cycles to pass a given point per unit of time (cycles per second), the SI unit of frequency is the hertz

question

frequency vs. wavelength

answer

the frequency and wavelength of light are inversely proportional to each other

question

energy vs. frequency

answer

energy and frequency are directly related

question

electromagnetic wave speed

answer

all electromagnetic waves travel in a vacuum at a speed of 2.998 x 10^8 m/s

question

speed of light formula

answer

speed of light (c) = frequency (v) x wavelength (?)

question

electromagnetic radiation

answer

includes radio waves, microwaves, visible light, ultraviolet waves, x-rays, and gamma rays.

question

spectrum

answer

range of wavelengths of electromagnetic radiation (red has the longest wavelength and longest frequency, violet has the shortest wavelength and shortest frequency)

question

electron absorption

answer

atoms absorb energy that raises electrons into higher energy levels and then lose the energy by emitting light when electrons return to lower energy levels

question

atomic emission spectrum

answer

the pattern formed when light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains, useful in identifying elements (ex. what stars are made of) (No two elements have the same emission spectrum)

question

ground state

answer

lowest possible energy of the electron, quantum number (n) = 1, a quantum of light in the form of light is emitted when the electron drops from a higher energy level to a lower energy level

question

Heisenberg Uncertainty Principle

answer

states that it is impossible to know exactly both the velocity and the position of a particle at the same time

question

Dmitri Mendeleev

answer

published the first version of what is now known as the periodic table in order of increasing atomic mass

question

Henry Moseley

answer

assigned atomic numbers to the elements and the periodic table was reordered into increasing atomic number in 1913

question

Periodic Law

answer

when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

question

reactivity of metals

answer

metals are more reactive on the left side of the periodic table, metals are more reactive towards the bottom of the periodic table

question

reactivity of nonmetals

answer

nonmetals are more less reactive on the left side of the periodic table, nonmetals are more reactive towards the top of the periodic table

question

metals

answer

good conductors of heat and electric current, make up 80% of all elements

question

nonmetals

answer

poor conductors of heat and electric current (carbon is an exception)

question

metalloids

answer

properties of both metals and nonmetals

question

alkali metals

answer

very reactive, group 1A on the periodic table of elements

question

alkaline earth metals

answer

reactive, group 2A on the periodic table

question

grouping based on electron configuration

answer

elements can be sorted into noble gases, representative elements, transition elements, or inner transition metals based on electron configuration

question

noble gas

answer

not very reactive at all, elements in group 8A of the periodic table

question

representative elements

answer

groups 1A and 7A because they display a wide range of physical and chemical properties

question

transition metal

answer

one of the group B elements where the s sublevel and d sublevel contain electrons

question

inner transition metal

answer

highest s sublevel and a f sublevel are occupied by electrons

question

trends in atomic size

answer

increases to the right and down the periodic table, the atomic size of an element will increase with the atomic number Cations are always smaller than the atoms from which they form (they lose electrons, of course they are going to be smaller) Anions are always larger than the atoms from which they form (they gain electron, therefore, they will be larger)

question

atomic radius

answer

one half of the distance between the nuclei of two atoms of the same element with the atoms are joined

question

ions

answer

an atom or a group of atoms with a positive or negative charge, form when electrons are transferred between atoms

question

cation

answer

ion with a positive charge, atoms that tend to lose a valence electron become a positive ion (cation)

question

anion

answer

ion with a negative charge, atoms that tend to gain a valence electron become a negative ion (anion) and usually end in -ide

question

ionization energy

answer

the energy required to remove an electron from an atom

question

trends in ionization energy

answer

increases from bottom to top and from left to right on the periodic table

question

shielding effect

answer

describes the attraction between an electron and the nucleus in any atom with more than one electron shell

question

Why does ionization energy increase as you either move up, or move to the right on the periodic table?

answer

The smaller the atomic radius the closer the electrons are to the nucleus. As you recall the nucleus is positively charged. This means it is going to require more energy to remove that electron.

question

trends in electronegativity

answer

increases up and to the right of the periodic table (excluding noble gases)

question

electronegativity

answer

the ability of an atom of an element to attract electrons when the atom is in a compound

question

What is the relationship between atomic radius and electronegativity? Why?

answer

The smaller the atomic radius the more electronegativity the atom has. The smaller the atomic radius indicates that the atom has fewer energy levels meaning that the valence electrons are closer to the positively charged nucleus. This allow the positively charged nucleus to have a larger impact on attracting electrons from other atoms.

question

valence electrons

answer

the electrons in the highest occupied energy level of an element's atoms, they correspond with the group numbers on the periodic table, usually the only ones used in chemical bonds

question

Lewis (electron) Dot Structures

answer

diagrams that show valence electrons as dots

question

Octet Rule

answer

when forming compounds, atoms tend to achieve the electron, configuration of a noble gas (which has eight valence electrons)

question

metallic atoms vs nonmetallic atoms

answer

metallic atoms tend to lose their valence electrons, while most nonmetals tend to gain valence electrons to form an octet

question

transition metal charges

answer

? charges of cations can vary ? some metals like silver do not reach the electron configuration of a gas ? charges above positive three are very uncommon

question

hallide ions

answer

ions formed when halogens gain an electron

question

ionic compounds

answer

compounds formed of cations and ions, are electrically neutral, generally form a metal and nonmetal

question

ionic bonds

answer

the electrostatic forces that hold ions together in ionic compounds

question

chemical formula

answer

show the kinds and numbers of atoms in the smallest representative unit of a substance

question

formula unit

answer

the lowest whole number ration of ions in an ionic compound, ex: H12O6 = H2O

question

properties of ionic compounds

answer

usually solid crystals at room temperature, generally have high melting/boiling points, can conduct electric current when melted or dissolved in water/aqueous solution, brittle

question

properties of covalent compounds

answer

exist as solids, liquids or gases, low melting/boiling points, don't conduct electricity at any state, don't dissolve in water

question

metallic bonds

answer

consist of the attraction of the free-floating valence electrons, for the positively charged metal ions (sea of moving electrons), these are the bonds that hold metals together, metals are arranged in very compact/orderly patterns

question

metallic bonding characteristics

answer

high melting/boiling point, high conductivity, malleable, ductile and have luster

question

alloys

answer

mixtures composed of two or more elements, at least on is a metal, ex: sterling silver, bronze, steel

question

covalent bond

answer

atoms held together by sharing electrons

question

molecule

answer

an electrically neutral group of atoms joined together by covalent bonds

question

diatomic molecules

answer

molecule consisting of two atoms

question

molecular compound

answer

a compound composed of molecules, tend to have low melting/boiling points

question

molecular formula

answer

shows the kinds and numbers of atoms present in a molecule or compound, not necessarily lowest whole number ratios

question

nature of covalent bonding

answer

when forming covalent bonds, electron sharing tends to occur so that atoms, with shared electrons included, attain the electron configuration of noble gases ? as you increase the number of bonds, the bond length decreases and the bond strength decreases

question

single covalent bonds

answer

atoms share one electron each

question

double covalent bonds

answer

when atoms share two electrons each

question

triple covalent bonds

answer

each atom shares three electrons

question

bond length

answer

the average distance between nuclei of two bonded atoms in a molecule

question

bond strength

answer

the degree to which each atom is joined to another in a chemical bond

question

dissociation energy

answer

the amount of energy required to break a bond, the higher the dissociation energy the stronger the bond

question

electron dot diagram

answer

show bonding by a way of dots

question

structural formuala

answer

shows bonding using dashes

question

unshared pair

answer

a pair of valence electrons that is not shared between atoms

question

resonance structure

answer

a structure that occurs when it is possible to write two or more valid electron dot formulas that have the same number of electron pairs for a molecule or ion

question

exceptions to the Octet Rule

answer

octet rule cannot be satisfied in molecules whose total number of valence electrons is an odd number, molecules in which an atom has fewer or more than a complete octet of valence electrons

question

molecular orbitals

answer

the model that shows that when two atoms combine, their atomic orbitals overlap

question

sigma bond

answer

bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting two atomic nuclei (caused by attraction of nuclei and electrons)

question

pi bonds

answer

are side by side overlap of atomic p orbitals

question

VSEPR Theory

answer

explains the three dimensional shape of a structure

question

linear (VSEPR shape)

answer

3 atoms, 180 degree angle

question

bent (VSEPR shape)

answer

3 atoms, 120 degree angle

question

lone pair of electrons

answer

refers to a pair of valence electrons that are not shared with another atom and is sometimes called a non-bonding pair

question

trigonal planar (VSEPR shape)

answer

4 atoms, 120 degree angle

question

pyramidal (VSEPR shape)

answer

unshared pair of electrons, 4 atoms, 109 degree angle

question

tetrahedral (VSEPR shape)

answer

4 atoms, 109.5 degrees

question

t shaped (VSEPR shape)

answer

4 atoms, 2 unshared pairs of electrons

question

square planar (VSEPR shape)

answer

5 atoms, 2 unshared pairs of electrons

question

nonpolar covalent bond

answer

when atoms in a covalent bond pull equally, the bonding electrons are shared equally

question

polar covalent bond

answer

a covalent bond between atoms in which the electrons are shared unequally, the more electronegative atom attracts electrons more strongly and gains a slightly negative charge, the less electronegative atom has a slightly positive charge

question

polar molecule

answer

one end of the molecule is going to be slightly positive and the other end will be slightly negative

question

dipole

answer

a molecule that has two poles, when polar molecules are placed between oppositely charged plates, they tend to become oriented with respect to the positive and negative plate, attraction between molecules are weaker than ionic and covalent bonds

question

dipole interactions

answer

occur when polar molecules are attracted to one other

question

London dispersion forces

answer

occur when moving electrons happen to be momentarily move on the side of a molecule closest to the neighboring molecule (very weak)

question

hydrogen bonds

answer

attractive forces in which a hydrogen bond covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom

question

order of strength of intermolecular forces

answer

1. hydrogen bonding 2. dipole 3. London dispersion forces

question

criteria for a chemical change

answer

1. precipitate formation 2. evolution of a gas 3. changes in energy

question

types of chemical reactions

answer

1. synthesis 2. decomposition 3. single replacement 4. double replacement 5. combustion

question

synthesis

answer

a chemical change in which two or more substances react to form a single new substance

question

decomposition

answer

a chemical change in which a single compound is broken down into two or more simpler products

question

single replacement

answer

a chemical change in which one element replaces a second element in a compound

question

double replacement

answer

a chemical change that involves an exchange of positive ions between two compounds, anions and cations switch places

question

combustion

answer

a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light

question

chemical equations

answer

a representative of a chemical reaction, the reactants are on the left are connected by an arrow with the formulas of the products on the right

question

catalyst

answer

a substance that speeds up a chemical reaction, written above the arrow in a chemical reaction, is neither a reactant or a product

question

coefficients

answer

small whole numbers that are placed in front of the formulas in an equation in order to balance it

question

balanced equation

answer

each side of the equation has the same number of atoms of each element and mass is conserved

question

skeleton equation

answer

simplest form of a chemical equation that does not have coefficients

question

rules on predicting products

answer

1. the compounds that form must be neutral in charge 2. DO NOT carry any subscripts over from the reactant side 3. balance your equation last

question

displacement recations

answer

? metals will not always replace other metals in a reaction due to their reactivity ? in order for one metal to replace another, the other metal must be more reactive than the one that is replacing (the same rule applies for halogens)

question

endothermic vs exothermic

answer

? If the element is MORE reactive than the one it is trying to replace then the reaction will occur and it will be exothermic ? If the element is LESS reactive than the one it is trying to replace then there will be no reaction and it will be endothermic

question

rules for double replacement reactions

answer

? not all double displacement reactions occur ? in order for a double replacement reaction to occur, both reactants must be soluble in water (if only one of the ions in a compound is soluble the compound will be at least moderately soluble) ? one product must be soluble, one product must be insoluble (the insoluble product is the precipitate and the precipitate will usually be a solid)

question

spectator ion

answer

an ion that appears on both sides of an equation and is not directly involved in the reaction

question

mole

answer

the amount of a substance that contains 6.022 x 10^23 representative particles of that substance

question

Avogadro's number

answer

the number of representative particles contained in one mole of a substance (6.022 x 10^23)

question

molar mass

answer

term used to refer to the mass of a mole of any substance

question

mole ratio

answer

a conversion factor deprived from the coefficients of a balanced chemical equation interpreted in terms of moles

question

stoichiometry

answer

the calculation of quantities in chemical reactions (the coefficients of a balanced equation indicates the relative number of moles of reactants and products in a chemical reaction)

question

stoichiometry steps

answer

1. balance the chemical equation 2. identify the given chemical ; measure and the unknown (to be found) chemical and measure 3. change the measure of the given chemical into moles 4. use the balanced chemical coefficients to form a ratio with the coefficient of the unknown chemical in the numerator, and the coefficient of the given chemical in the denominator, multiply the given moles by this ratio to find the moles of unknown chemical 5. change the unknown number of moles to the measure that was requested

question

standard temperature and pressure (STP)

answer

the conditions under which the volume of a gas is usually measured (1 mole of any gas at STP occupies a volume of 22.4 L)

question

limiting reagent

answer

determines the amount of product that can be formed in a reaction, the reaction occurs until the limiting reagent is up

question

excess reagent

answer

the reactant that is not completely used up in a reaction

question

compressiblity

answer

a measure of how much the volume of matter decreases under pressure (gases are more easily compressed than solid or liquids because of the space between their particles)

question

variables used to describe a gas

answer

1. pressure KPa (kilopascals) 2. volume L (liters) 3. temperature K (Kelvin) 4. number of moles (n)

question

kinetic molecular theory

answer

1. The volume occupied by the individual particles of a gas is negligible compared to the volume of the gas itself. 2. The particles of an ideal gas exert no attractive forces on each other or their surroundings. 3. Gas particles are in a constant state of random motion and move in straight lines until they collide with another body. 4. The collisions exhibited by gas particles are completely elastic; when two molecules collide, total kinetic energy is conserved. 5. The average kinetic energy of gas molecules is directly proportional to absolute temperature only; this implies that all molecular motion ceases if the temperature is reduced to absolute zero.

question

gas laws

answer

1. Boyle's Law 2. Charles' Law 3. Gay-Lussac's Law 4. Dalton's Law 5. Ideal Gas Law

question

Boyle's Law

answer

states that for a given mass of gas at constant temperature, the volume of gas varies INVERSELY with pressure (equation: P1V1 = P2V2)

question

Charles' Law

answer

states that the volume of a fixed mass of gas is directly proportional to its Kelvin temperature (equation: V1/V2 = V2/T2)

question

Gay-Lussac's Law

answer

states that the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant (equation: P1/T1 = P2/T2)

question

Combined Gas Law

answer

allows calculations to be done when gas is constant (equation: P1 x (V1/T1) = P2 x (V2/T2)

question

Ideal Gas Law

answer

law stating that allows problems involving pressure, temperature and volume to be solved (equation: PV = nRT)

question

ideal gas

answer

a hypothetical gas whose molecules exhibit no interaction and

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