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Chemistry > Final Review > Flashcards

Final Review Flashcards

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1
Q

the more electronegative atom is assigned…

A

ALL the shared electrons

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2
Q

the less electronegative atom is assigned…

A

none of the shared electrons

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3
Q

each atom in a bond is assigned…

A

ALL of its unshared electrons

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4
Q

valence (e-) - [# shared (e-) + # unshared (e-) ] =

A

Oxidation Number

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5
Q 
the charge an atom would have if all electrons were shared equally--
# of valence (e-)  -  (# unshared valence e- + 1/2# of shared e-)
A

Formal charge

*bonding electrons are shared equally by the atoms

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6
Q

the energy required to separate 1 mol of an ionic solid into gaseous ions; measure of the strength of an ionic bond
Also ~ (charge A x charge B) / distance

A

Lattice Energy

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7
Q

the # of electron pairs being shared by a given pair of atoms
= 1/2[(# e- in bonding MO) - (# e- in antibonding MO)]

A

Bond order (a single bond has 1 pair so BO = 1)

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8
Q

the energy needed to overcome the attraction between the nuclei and the shared electrons;
* the higher the bond energy the stronger the bond

A

Bond energy

*bond energy DECREASES down a group and INCREASES across a period

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9
Q

the distance between the nuclei of the bonded atoms

A

Bond length

*the shorter the distance the stronger the bond

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10
Q

bond length increases…

A

DOWN a group and…

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11
Q

bond length decreases…

A

ACROSS a period

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12
Q

the heat releases or absorbed during a chemical change is due to differences between the bond energies of reactants and products

A

deltaH(rxn) = sum[deltaH(reactant bonds broken)] + sum[deltaH(product bonds formed)]

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13
Q

ability of an atom to attract the shared electron pair

A

electronegativity

*atoms with lowest EN are placed in the middle

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14
Q

_______have the same relative placement of atoms but different locations of bonding and lone electron pairs

A

resonance structures

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15
Q

a species which can be depicted by more than one valid Lewis structure =

A

resonance hybrid

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16
Q

AXmEn

A

A = central atom
X = surrounding atom
E = nonbonding valence-electron group
(m and n are integers)

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17
Q

______have high IEs and highly negative EAs

*they tend to attract electrons strongly and form negative ions

A

Reactive nonmetals

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18
Q

______have low IEs and slightly negative EAs

*tend to lose electrons easily and form positive ions

A

Reactive metals

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19
Q

______have very high IEs nd slightly positive EAs

*they tend to neither gain or lose electrons

A

Noble gases

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20
Q

n =

A

orbital energy

positive intergers 1, 2, 3…

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21
Q

l =

A

orbital shape; positive integers from 0 to n-1

s, p, d, and f

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22
Q

m sub l =

A

integers from -l to 0 to l

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23
Q

m sub s =

A

electron spin direction

+ or - 1/2

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24
Q

the # of electrons lost or gained by an atom

A

Oxidation Number

  • bonding electrons are transferred to the more electronegative atom
  • always the same
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25
Q

the energy change that occurs when 1 mol of electrons is added to 1 mol of gaseous atoms or ions

A

Electron Affinity

  • low EA–> form cations
  • high EA–> form anions
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26
Q

the energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions
*tends to DECREASE down a group and INCREASE across a period

A

Ionization energy

  • low IE–> form cations
  • high IE –> form anions (except noble gases)
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27
Q

theory that a covalent bond forms when the orbitals of 2 atoms overlap and a pair of electrons occupy the overlap region
the space formed by the overlapping orbitals can accommodate a max of 2 electrons with opposing spins
*the greater the overlap, the stronger the bond

A

Valence Bond Theory

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28
Q

A molecule is polar if…

A

it contains 1 or more polar bonds and

the individual bond dipoles do not cancel

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29
Q

anything that has both mass and volume

A

matter

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30
Q

the types and amounts of simpler substances that make up a sample of matter

A

composition

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31
Q

the characteristics that give each substance a unique identity

A

properties

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32
Q

properties a substance shows by itself without interacting with another substance, i.e. color, melting point, boiling point, density

A

physical properties

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33
Q

properties a substance shows as it interacts with or transforms into other substances, i.e. flammability, corrosiveness

A

chemical properties

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34
Q

has a fixed shape and volume

A

solid

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35
Q

has a varying shape that conforms to the shape of the container but a fixed volume; has an upper surface

A

liquid

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36
Q

has no fixed shape or volume and therefore does not have a surface

A

gas

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37
Q

the ability to do work

A

energy

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38
Q

the energy due to the position of an object

A

potential energy

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39
Q

the energy due to the movement of an object

A

kinetic energy

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40
Q

potential energy + kinetic energy

A

Total energy

41
Q

1 degree Celsius =

A

1 Kelvin

42
Q

1 degree Celsius/1 Kelvin =

A

1.9 degrees Farenheit

43
Q

“The total mass of substances present does not change during a chemical reaction

A

Law of Conservation of Mass

44
Q

If elements A and B react to form 2 compounds, the different masses of B that combine with a fixed mass of A can be expressed as a ration of small whole numbers

A

Law of Multiple Proportions

45
Q

X =

A

Atomic symbol of the element

46
Q

Z =

A

atomic number (# of protons in nucleus)

47
Q

A =

A

mass number (A = Z + N)

48
Q

N =

A

of neutrons in nucleus

49
Q

atoms of an element with the same number of protons but a different number of neutrons

A

Isotopes

*they have the same Z# but different A #’s

50
Q

the basic unit of an element or covalent compound consisting of 2 or more atoms bonded by the sharing of electrons
*most covalent substances consist of these

A

Molecule

51
Q

a single atom or covalently bonded group of atoms that has an overall electrical charge

A

Ion

*Refer to formula mass, not molecular mass

52
Q

Molecular mass =

A

sum of the atomic masses

*to 4 sig figs

53
Q

the amount of substance that contains the same number of entities–(atoms, ions, molecules, electrons, formula units or any particle type)–as there are atoms in exactly 12 g of carbon-12

A

mole (mol)
–Avogadro’s # (N):
= 6.0222 x 10^23 entities (to 4 sig figs)

54
Q

the mass of a substance per mole of its entities

A

Molecular mass

55
Q

the simplest formula for a compound; shows the lowest whole # of moles and gives the relative # of atoms of each element present

A

Empirical formula

56
Q

shows the ACTUAL # of atoms of each element in a molecule of the compound

A

Molecular formula

57
Q

consists of 1 or more solutes dissolved in a solvent

A

solution

58
Q

given by the quantity of solute present in a given quantity of solution;
expressed by ‘M’ = moles of solute/L of solution

A

concentration

Molarity

59
Q 
common compounds of group 1A (Li+ Na+ K+)
NH4+
common nitrates (NO3-) 
acetates (CH3COO- or C2H3O2-)
most perchlorates (ClO4-)
common chlorides (Cl-), bromides (Br-), 
Iodides (I-) and common fluorides (F-)
*except Pb2+, Ag+, Cu+ Hg2+ and group 2A
common sulfates (SO2^2-) *except Ca2+ Sr2+ Ba2+ Ag+ and Pb2+
A

Soluble Ionic Compounds

60
Q

all common metal hydroxides–except group 1A and larger members of group 2A beginning with Ca2+
all common carbonates (CO3^2-) and phosphates (PO4^3-)–except group 1A and NH4+
all common sulfides–*except group 1A, 2A and NH4+

A

Insoluble Ionic Compounds

61
Q

a substance that produces H+ ions when dissolved in H2O

A

acid

62
Q

a substance that produces OH- ions when dissolved in H2O

A

base

63
Q

also called a neutralization reaction

A

acid-base reaction

64
Q

the loss of electrons

A

oxidation

65
Q

loses electrons and is oxidized

A

reducing agent

66
Q

gains electrons and is reduced

A

oxidizing agent

67
Q

the gain of electrons

A

reduction

68
Q

electron transfer, oxidation and reduction occur together

A

a redox reaction

69
Q

2 or more reactants combine to form a new compound: x + y –> z

A

combination reaction

70
Q

z –> x + y

A

decomposition reaction

71
Q

ab + cd –> ac + bd

A

double displacement

72
Q

x + yz –> xz + y

A

single displacement

73
Q

the process of combining with O2

A

Combustion

74
Q

when orbitals of equal energy are available, the lowest energy electron configuration has the max # of unpaired electrons with parallel spins

A

Hund’s Rule

75
Q

exhibits linear relationships among the variables of pressure, volume, temperature, and amount (moles)

A

idea gas

76
Q

q (+) =

A

system GAINS heat

77
Q

w (+) =

A

work done ON system

78
Q

q (-) =

A

system RELEASES heat

79
Q

w (-) =

A

work done BY system

80
Q

1 kg * m^2 / s^2 =

A

1 J (joule)

81
Q

1 calorie =

A

4.184 J

82
Q

Enthalpy and chemical change:

A

deltaH = deltaE(q+w) + deltaPV = q
(deltaH ~ deltaE)
*for reactions without gases/where total moles don’t change/when q is much > deltaPV

83
Q

q = c x m x deltaT

A

q- heat lost or gained
c - specific heat capacity
m- mass in grams
deltaT- T(final) - T(initial)

84
Q

the enthalpy change of an overall process is the sum of the enthalpy changes of its individual steps

A

Hess’s law

deltaH overall = deltaH1 + deltaH2 +……+ deltaHn

85
Q

cycles per second =

A

frequency

86
Q

the distance a wave travels in one cycle

A

wavelength

87
Q

the height of a wave crest or depth of a trough =

A

amplitude

88
Q

the speed of light (c) is constant:

= 3.00 x 10^8 m/s (in a vacuum)

A

c = v x h

89
Q

a solid object emits visible light when it is heated to about 1000K =

A

blackbody radiation

90
Q

color is related to________ & _________

A

wavelength and frequency

91
Q

temperature is related to __________

A

energy

92
Q

E = nhv …

A 
E = energy
n = a positive integer
h = Planck's constant
v = frequency
93
Q

It is not possible to know both the position and momentum of a moving particle at the same time
deltaX * m * deltaU >/= h/4pi
x = position
u - speed

A

Heisenberg’s Uncertainty Principle

*the more accurately we know the speed, the less accurately we know the position, and vice versa

94
Q

Intensive

A

a physical property that doesn’t depend on the size or amount of material in the system/on outside variables (i.e. hardness)

95
Q

extensive

A

a physical property that is proportional to the amount of material/size of system (i.e. mass and volume)

96
Q

how contact lenses focus light

A

refraction

97
Q

______

A

dispersion

98
Q

separating through slits when an obstacle is met

A

diffraction

Chemistry (6 decks)

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