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Chem Flashcards

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1
Q

_____ describes the orientation of the orbital

A

magnetic quantum number

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2
Q

mass number

A

protons + neutrons

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3
Q

number of protons in an element

A

atomic number

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4
Q

an atom with the same number of protons but a different number of neutrons

A

isotope

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5
Q

positively charged ions (losses electrons)

A

cations

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6
Q

negatively charged ions (gains electrons)

A

anions

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7
Q

how to find the molecular mass

A

the sum of the avg atomic mass for each element

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8
Q

avogadros number

A

6.022 x 10^23

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9
Q

molar mass

A

of g / 1 mol

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10
Q

specific isotope of an element

A

nuclide

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11
Q

daltons three laws

A

law of conservation of mass
law of definite proportions
law of multiple proportions

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12
Q

mass cannot be created or destroyed in ordinary chemical and physical changes

A

law of conservation of mass

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13
Q

a chemical compound always contains the same elements in exactly the same proportions by weight or mass

A

law of definite proportions

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14
Q

when two elements combine to form two or more compounds, the mass of one element that combines with the given mass of the other is in the ratio of small whole numbers

A

law of multiple proportions

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15
Q

what did the cathode-ray tube experiment by JJ Thomas discover?

A

tiny negative charged particles

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16
Q

What experiment by Robert Mulikan discovered the charge of electrons?

A

oil drip experiment

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17
Q

what did the gold foil experiment by Rutherford, Geiger, and Marsden discover?

A

nucleus of an atom

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18
Q

what discovery did the experiment “a-particle at Be” by James Chadwick do?

A

the discovery of neutrons

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19
Q

most of the atoms mass and all its positive charge are contained in a small core called what

A

the nucleus

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20
Q

the volume of an atom is mostly what

A

empty space

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21
Q

what provides stability in the nucleus

A

neutrons

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22
Q

3 types of hydrogen isotopes

A

protium deuterium and tritium

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23
Q

when the frequency and the energy are low, the wavelength is what?

A

the wavelength is long

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24
Q

what happens when the energy of a photon increases?

A

the wavelength gets shorter

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25
Q

the distance between adjacent crest of a wave

A

wavelength

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26
Q

the more frequently a wavelength will pass a given point, the wavelength will be what

A

shorter

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27
Q

energy is released or absorbed in discrete packets of energy

A

plancks hypothesis

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28
Q

very tiny packet of radiant energy

A

photon

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29
Q

plancks constant

A

6.626 x 10^-34 Jxs

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30
Q

inversely proportional to wavelength

A

energy

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31
Q

group 1,2, and 13-18 on the periodic table are called

A

main group elements

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32
Q

group 3-12 on the periodic table are called

A

transition metals

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33
Q

group 1 are called

A

alkali metals (except H)

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34
Q

group 2 are called

A

alkaline metals

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35
Q

group 17 are called

A

halogens

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36
Q

group 18 is called

A

noble gases

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37
Q

period 6 ( elements 58-71) are called

A

lanthanides

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38
Q

period 7 ( elements 90-103) are called

A

actinides

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39
Q

d 10^-1

A

deci

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40
Q

c 10^-2

A

centi

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41
Q

m 10^-3

A

milli

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42
Q

u 10^-6

A

micro

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43
Q

n 10^-9

A

nano

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44
Q

p 10^-12

A

pico

45
Q

What is the rule surrounding significant figures in scientific notation?

A

all digits before the multiplication symbol are significant

46
Q

What is the exception to significant figure rules?

A

if a value is a whole number, ends in a zero, with no decimal then the ending zeros are NOT significant (ex: 96,500)

47
Q

When do you apply significant figure rules?

A

end of calculations

48
Q

subtraction/addition rule for significant figures

A

the number of decimal places in the final answer is equal to the number with he least amount of decimal places

49
Q

multiplication/division rule for significant figures

A

the number of sig figs is equal to the LEAST amount of total sig figs in the problem; look at the entire number

50
Q

When do you not consider sig figs?

A

when using exact/known conversion factors

51
Q

Based on the data collected from Thomson’s cathode ray experiment, he suggested the:

A

plum pudding model

52
Q

What did Thomson lack in proving his plum pudding model?

A

evidence

53
Q

Fully disproved the plum pudding model by shooting a-particles at an ultra thin sheet of gold foil and measured the angles of scattering

A

Rutherford’s Gold Foil Experiment

54
Q

The gold foil experiment determined that the gold atom has a:

A

positively charged center, orders of magnitude smaller than the total mass of an atom (most of the atom is empty space)

55
Q

The gold foil experiment helped to shape and develop what model of the atom?

A

nuclear model of the atom

56
Q

3 parts of nuclear theory

A
  1. most of the atom’s mass and all its positive charge are contained in a small core called a nucleus
  2. due to electros being spaced out within the cloud, most of the volume of an atom is just empty space
  3. there are as many negatively charged electrons outside the nucleus as there are positively charged particles within the nucleus. this atom is electrically neutral
57
Q

Rutherford and Chadwick discovered the unaccounted mass of an atom was due to what?

A

neutrons

58
Q

the average atomic mass is the:

A

weighted average of all isotopes in the sample (amu=unit)

59
Q

Where can you find an element’s atomic mass on a periodic table?

A

below the element symbol

60
Q

an atom that gains or loses an electron

A

ion

61
Q

a positive charged ion means an atom

A

lost electrons

62
Q

a negatively charged ion means an atom

A

gains electrons

63
Q

In the very market 1900s German physicist Max Planck proposed that electromagnetic radiation is not:

A

continuous by its quantized

64
Q

Planck’s hypothesis said energy is

A

released or absorbed in discrete packets of energy

65
Q

Back the Planck formulated the idea of quantized energy, he had no experimental evidence to support its existence. However, Albert Einstein came along and supplied the evidence through his Nobel prize winning experiment the:

A

photo electric effect

66
Q

What did Einstein observe?

A

many metals emit photo electrons when light shines upon them

67
Q

E = hv

A

Energy = Planck’s constant x frequency

68
Q

E = hc/lambda

A

Energy = planck’s constant x speed of light / wavelength

69
Q

Energy is what relation to wavelength?

A

inversely proportional

70
Q

What did Bohr’s model explain?

A

why hydrogen atoms lose and gain discrete quanta of energy (photon) and why hydrogen’s electron does not spiral into the nucleus

71
Q

What are two general concepts with the Bohr orbits?

A

the greater the n value, the higher the energy; the energy difference between orbitals decreased with increasing values of n

72
Q

when electrons move up they what energy? (1-4) (3-4)

A

absorb

73
Q

when electrons go down they what energy? (2-1) (4-2)

A

emit

74
Q

an atomic model in which electrons are treated as waves; also called the wave mechanical model of the atom

A

the quantum model of the atom

75
Q

states that we cannot know both the position and speed of an electron at the same time

A

Heisenberg’s uncertainty principle

76
Q

Study of physics at the atomic level where energy is quantized in discrete, rather than continuous, levels.

A

quantum mechanics

77
Q

electrons do not travel around the nucleus in orbits, but instead they exist in regions of probability called

A

orbitals

78
Q

Just like the bohr model, shells with a larger principal quantum number are:

A

farther from the nucleus and have higher energies

79
Q

a positive whole number that indicates the main energy level/shell (n=1, 2, 3, 4,…)

A

principal quantum number (n)

80
Q

What does it mean if electrons have the same n value

A

they are in the same shell

81
Q

l = 0

A

s

82
Q

l = 1

A

p

83
Q

l = 2

A

d

84
Q

l = 3

A

f

85
Q

Orbitals with the constant value of n and l are in the:

A

same sub shell and have the same energy

86
Q

electrons in orbitals behave like the Earth spinning on an axis. the electron can only exist in one of two possible spin states which creates what?

A

magnetic fields

87
Q

An atomic orbital may describe at most two electrons, each with opposite spin direction

A

pauli exclusion principle

88
Q

The chemical behavior of an atom is determined by the distribution of electrons in electron shells

A

electron distribution

89
Q

the point at which the electron probability is zero

A

node

90
Q

the arrangement of electrons in an atom

A

electron configuration

91
Q

condensed electron configurations are useful because they elevate the electron configuration of the what?

A

core elements

92
Q

core electrons are not involved in the chemistries of the elements, so they are of less interest. Instead, chemists are more interested in what?

A

valence electrons

93
Q

electrons in the outermost shell

A

valence electrons

94
Q

What are the two exceptions to Aufbau rule?

A

chromium (Cr) and Copper (Cu) and they translate down their groups (6 and 11); they don’t fill up their 4s orbital

95
Q

electron configuration of chromium

A

[Ar] 4s^1 3d^5

96
Q

electron configuration of copper

A

[Ar] 4s^1 3d^10

97
Q

How do you write electron configurations for cations?

A

remove electrons with the highest energy level (n)

98
Q

unpaired electrons, attracted to magnetic field

A

paramagnetic

99
Q

all electrons are paired; not attracted to magnetic field

A

diamagnetic

100
Q

generally, it increases from top to bottom in a group (energy levels increases) and decreases from left to right across a period (# of protons increases, higher nuclear attraction)

A

the size of atoms (atomic radii)

101
Q

The amount of energy required to remove an electron from an atom

A

ionization energy

102
Q

the amount of energy required to remove the first electron

A

first ionization energy (IE1)

103
Q

in general, they increase from left to right across a period (more protons, greater Zeff) and decrease as you move down a group (larger atomic size, electrons aren’t pulled as close to the nucleus)

A

first ionization energies for main group elements

104
Q

What is an exception #1 to first ionization energy?

A

between groups 2 and 13 elements in the 2 and 3 row there is a decrease because group 13 will lose a p electron when they ionize and group 2 will lose a p electron when they ionize

105
Q

When do ionization energies drastically increase?

A

when you begin removing core electrons

106
Q

in general, the larger the radius of the atom, the greater ability to

A

lose electrons

107
Q

the measure of the ability of an atom to attract an electron within a chemical bond

A

electronegativity

108
Q

the energy change that occurs when an electron is acquired by a neutral atom

A

electron affinity

Chem (4 decks)

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