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CHM 2045 > CHM 2045 - Final > Flashcards

CHM 2045 - Final Flashcards

1
Q

Most of the volume of an atom is empty space, throughout which are dispersed _________.

A

electrons

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2
Q

Cathode ray tubes were used in the discovery of ________.

A

electrons

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3
Q

The law of conservation of mass states that in a chemical reaction, matter is never ….?

A

created nor destroyed

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4
Q

Most of an atom’s mass and all of its positive charge are contained in the atom’s _______.

A

nucleus

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5
Q

Nonmetals tend to gain electrons to form _______.

A

anions

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6
Q

The number of ______ in an atom defines its identity.

A

protons

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7
Q

The percentage of a particular isotope of an atom found in a natural sample of that element is called the _______ ________.

A

natural abundance

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8
Q

______ are good conductors of heat and electricity, often shiny, ductile, malleable, and tend to lose electrons when undergoing a chemical change.

A

Metals

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9
Q

One of the postulates of John Dalton’s atomic theory is that each element is composed of tiny, indestructible particles called _____.

A

atoms

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10
Q

______ are positively charged ions.

A

Cations

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11
Q

Avogadro’s number is the number of atoms contained in exactly 12g of ______-__.

A

carbon-12

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12
Q

The average mass of a molecule is the _______ _____.

A

formula mass

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13
Q

A(n) ________ reaction is a reaction in which a substance combines with oxygen to form carbon dioxide.

A

combustion

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14
Q

A(n) ______ bond typically occurs between a metal and a non-metal.

A

ionic

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15
Q

The _______ formula gives the number of atoms of each element in a molecule of a compound.

A

molecular

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16
Q

_______ compounds are compounds that contain only two elements.

A

Binary

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17
Q

The _____ _______ composition of an element is that element’s percentage of a compound’s total mass.

A

mass percent

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18
Q

A(n) _______ bond occurs between two non-metals.

A

covalent

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19
Q

Many molecular elements exist as ________ molecules.

A

diatomic

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20
Q

Organic compounds that contain only carbon and hydrogen are called __________.

A

hydrocarbons

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21
Q

The species that limits the amount of product that is formed in a chemical reaction is the ________ _______.

A

limiting reactant

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22
Q

______ reactions are those in which electrons are transferred from one species to another.

A

Redox

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23
Q

When a species is dissolved in water but does not form a solution that conducts electricity, it is called a(n) ___________.

A

nonelectrolyte

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24
Q

The ______ _____ is a numerical measure of the relationship between the actual yield and the theoretical yield.

A

percent yield

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25
Q

A reaction in which two solutions combine to form a solid is called a(n) ________ reaction.

A

precipitation

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26
Q

The numerical relationships between chemical amounts in a balanced reaction are called reaction ___________.

A

stoichiometry

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27
Q

The sum of oxidation states of all atoms in an ion is equal to the ____ charge.

A

ion

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28
Q

________ ions are species that are not involved in the chemistry of a solution phase reaction.

A

Spectator

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29
Q

A(n) _______ _________ is a species that dissociates completely in a solution to form ions.

A

strong electrolyte

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30
Q

Dalton’s law of _______ ______ states that the total pressure of a gas sample is equal to the sum of the partial pressures of its components

A

partial pressures

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31
Q

The average distance that a particle can travel in between collisions is called its _____-____-____.

A

mean-free-path

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32
Q

The average kinetic energy of a particle is proportional to its _________ in units of ______.

A

temperature, Kelvin

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33
Q

_______ is the force exerted per unit area by gas particles as they strike the walls of a container.

A

Pressure

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34
Q

Pressure and volume are ________ proportional.

A

inversely

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35
Q

A mercury barometer is a device that measures pressure in units of _____.

A

mmHg

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36
Q

The molar volume of an ideal gas at STP is always ____ L

A

22.4

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37
Q

How do you calculate mole fraction?

A

Xa = na/nTotal

Xa = pa/pTotal

38
Q

How do you calculate partial pressure?

A

Pa = Xa(Ptotal)

39
Q

How do you calculate density?

A

D = P(MM)/RT

40
Q

The SI units of energy are the _____.

A

joule

41
Q

1 cal = _____ J

A

4.184

42
Q

1 KJ = _____ J

A

1000J

43
Q

A(n) _______ is defined as the amount of energy required to raise the temperature of 1g of water by exactly 1ºC.

A

calorie

44
Q

A ______ function is one that depends only on the initials and final values, but not on the manner in which the system was prepared.

A

state

45
Q

When heat is absorbed by a system, the sign of delta H is _______.

A

positive

46
Q

A positive value of work is obtained when work is done ___ the system.

A

on

47
Q

The measure of a substance’s intrinsic capacity to absorb heat is called its _____ ________.

A

heat capacity

48
Q

When a closed system expands, the sign of work is ________.

A

negative

49
Q

An ________ reaction is one that absorbs heat from its surroundings.

A

endothermic

50
Q

The phenomenon of light bending around an obstacle or slit is called ________.

A

diffraction

51
Q

The ________ quantum number determines the orientation of an orbital

A

magnetic

52
Q

Delta E = __ + __

A

Detla E = q + v

53
Q

q = __ x __ x __

A

q = m x cs x detla T

54
Q

w = -__ x __

A

w = -p x delta V

55
Q

1 L x atm = _____ ?

A

101.3 J

56
Q

qrxn = - ( __ x __ x __ )

A

qrxn = - (m x cs x delta T)

57
Q

Delta Hrxn = ____/____

A

Delta Hrxn = qrxn/mole

58
Q

_________ radiation is a type of energy embodied in oscillating electric and magnetic fields.

A

Electromagnetic

59
Q

A _____ is a point where the wave function goes through zero.

A

node

60
Q

The highest energy region of the electromagnetic spectrum is _____ ______.

A

gamma rays

61
Q

__________ _______ occurs when two waves travel in phase with on another.

A

Constructive interference

62
Q

Energy is _______ from an atom when an electron moves to a lower energy level.

A

emitted

63
Q

The ________ uncertainty principle relates the uncertainty in an electron’s position to the uncertainty in its velocity.

A

Heisenberg

64
Q

The more certainly you know a given property, the less certain you know its __________ property.

A

complementary

65
Q

Which quantum number determines the overall size and approximate energy of an orbital?

A

Principal quantum number

66
Q

Which quantum number primarily determines the shape of the orbital?

A

Angular momentum quantum number

67
Q

The __________ ______ is the observation that many metals emit electrons when light is shined upon them.

A

photoelectric effect

68
Q

v = __/__

A

v = c/lamda

69
Q

1m = 1^ ? nm?

A

1m = 1^9 nm

70
Q

h = _______ (Plank’s constant)

A

6.626x10^-34 J/s

71
Q

E = __ x __

A

E = hv

72
Q

E could also equal….?

A

E = hc/lamda

73
Q

E photon = _____/______

A

E photon = E total/# photons

74
Q

photon’s = ______/______

A

photons = E pulse/E photon

75
Q

De Broglie Wavelength

Lamda = __/__ x __

A

Lamda = h/mv

*the mass must be in kg

76
Q

Excited electron…from low “n” to high “n” ______ a photon.

A

absorbs

77
Q

Relaxed electron…from high “n” to low “n” ______ a photon.

A

emits

78
Q

Wavelength is _______ proportional to frequency.

A

inversely

79
Q

The lowest energy state of an atom is its ______ ______.

A

ground state

80
Q

_______ are charged species that are much smaller than their corresponding atoms.

A

Cations

81
Q

An element with unpaired electrons is considered ___________.

A

paramagnetic

82
Q

The effective nuclear charge differs from the actual nuclear charge due to ________.

A

shielding

83
Q

______ ________ principle: Implies that each orbital can have a maximum of only two electrons , with opposing spins.

A

Pauli Exclusion

84
Q

_____ ______: When filling degenerate orbitals, electrons fill them singly first, with parallel spins.

A

Hund’s Rule

85
Q

The _________ energy is the energy required to remove an electron from an atom or ion in the gaseous state.

A

ionization

86
Q

Degenerate orbitals have the same ______.

A

energy

87
Q

The ability of an atom of attract electrons to itself in a chemical bond is called ___________.

A

electronegativity

88
Q

The ______ ______ of an atom is the charge it would have if all the bonding electrons were shared equally between the atoms.

A

formal charge

89
Q

How do you calculate formal charge?

A

F.c = ve - lone pairs - 1/2(bonding pairs)

90
Q

Expanded octets occur for elements in the ______ row or below.

A

third

91
Q

The lattice energy ________ when the size of the cation increases.

A

decreases

CHM 2045 (1 decks)

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