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Chemistry 101 > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

What is an element

A

consist of only one kind of atom, cannot be broken down

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2
Q

What is a compound

A

two or more elements chemically bonded together into molecules/extended structures

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3
Q

Daltons law of conservation of mass

A

total mass remains constant in a reaction

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4
Q

Daltons law of constant (definite) composition

A

all samples of a given compound consist of the same mass fraction

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5
Q

daltons law of multiple proportions

A

In different compounds of the same elements, the mass of combining the elements can be expressed in simple whole ratios

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6
Q

Who discovered the existence of negatively charged particles (electrons)

A

Thomson; also made plum-pudding model

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7
Q

Who did the oil drop experiment

A

Millikan

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8
Q

What is Rutherford’s Scattering Experiment

A

Metal foil shot by alpha particles, where some got deflected backward by a positive charge (nucleus)

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9
Q

The 3 subatomic particles

A

proton, neutron, electron

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10
Q

what does Z stand for in atomic notation

A

Atomic number (protons)

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11
Q

what does a stand for in atomic notation

A

mass number (protons + neutrons)

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12
Q

What is an isotope

A

The same number of protons (Z) but differ in mass number (A)

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13
Q

What group are the alkali metals

A

group 1, except H

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14
Q

What group are the alkaline earth metals

A

group 2

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15
Q

cation

A

positive ion, electron removed

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16
Q

anion

A

negative ion, electron added

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17
Q

what is a binary acid

A

contains no oxygen. hydro___ic acid

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18
Q

name this acid: HCN (aq)

A

hydrocyanic acid

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19
Q

Name this acid: HF (aq)

A

hydrofluoric acid

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20
Q

name this acid: H2S

A

hydrosulfuric acid

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21
Q

what is an oxyacid

A

contains H+O+nonmetal. name depends on the oxoanion

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22
Q

What is the oxyacid name when oxoanion is hypo___ite

A

hypo___ous acid

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23
Q

what is the oxyacid name when oxoanion is ___ite

A

___ous acid

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24
Q

what is the oxyacid name when oxoanion is ___ate

A

___ic acid

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25
Q

what is the oxyacid name when oxoanion is per__ate

A

per___ic acid

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26
Q

absorption

A

excitation from a lower allowed energy level to a higher allowed energy level

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27
Q

emission

A

relaxation from a higher allowed energy level to a lower allowed energy level (often ground level)

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28
Q

what is a ground state

A

the electron is in the first orbit (n=1)

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29
Q

what is ionization energy

A

The energy needed to completely remove the electron from the nucleus (n=infinity)

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30
Q

Is energy positive or negative in absorption

A

positive

31
Q

Is energy positive or negative in emission

A

negative

32
Q

Is energy positive or negative in ionization

A

positive

33
Q

Infrared series (infrared radiation)

A

when electrons drop from outer orbits (n=4/5) to n=3

34
Q

visible series (visible radiation)

A

when electrons drop to n=2 orbit (first excited state)

35
Q

ultraviolet series (UV radiation)

A

when electrons drop to the n=1 orbit (ground state)

36
Q

how are energy and wavelength related

A

inversely; smallest energy is longest wavelength

37
Q

how are a photon’s momentum and wavelength related

A

as momentum decreases, wavelength increases

38
Q

probability contour

A

the shape that defined the volume around the nucleus where the electron spends most of it’s time

39
Q

how to calculate the number of radial nodes

A

n-l-1

40
Q

what is the n quantum number in each orbital

A 
row of periodic table, starting at:
s=1
p=1
d=3
f=4
41
Q

what is the l quantum number in each orbital

A

s=0
p=1
d=2
f=3

42
Q

what is the ml quantum number

A

s=0
p= -1 to +1
d= -2 to +2
f= -3 to +3

43
Q

what shape is the s orbital

A

big sphere

44
Q

what shape is the p orbital

A

dumbbell shape

45
Q

what shape is the d orbital

A

clover type thing, nodal planes lie between the orbital lobes

46
Q

how to find number of angular nodes

A

given by l

47
Q

how to find total number of nodes

A

n-1

48
Q

Pauli’s Exclusion Principle

A

no two electrons can have all four quantum numbers alike

49
Q

What is Zeff

A

an effective nuclear charge (the nuclear charge and electron actually experiences due to shielding electrons

50
Q

Greater nuclear charge ___ orbital energy

A

lowers

51
Q

electron-electron repulsion _____ orbital energy

A

raises

52
Q

electrons in higher n are shielded from the full nuclear charge so they have ___ energy

A

higher

53
Q

orbitals with good penetration have ____ energy

A

lower

54
Q

order the orbitals from least shielding/penetration to most shielding/penetration

A

f,d,p,s

55
Q

order the orbitals in order from lowest energy to highest energy

A

s,p,d,f

56
Q

Hunds rule

A

when there are orbitals of equal energy, maximize unpaired spins first before doubling up

57
Q

Cr and Cu have what

A

anomalous configurations, attributed to special stability of 3d subshells (doesn’t follow the normal way fo writing quantum) Also includes Cr, Cu, Mo, Ag, Au

58
Q

How do transition metals lose electrons to form cations

A

s electrons are removed before the d electrons since d has a much lower energy

59
Q

paramagnetic

A

unpaired electrons

60
Q

diamagnetic

A

all electrons paired

61
Q

Compare the sizes of Li and Li+

A

cations smaller than atoms
Zeff increases as there is a net positive charge
Radius decreases

62
Q

Compare the sizes of F and F-

A

anions are larger than atoms
Zeff decreases as there is a net negative charge
radius increases

63
Q

What is the periodic trend of ionic size

A

down a group: ionic size increases

across a period: anion size decreases with decreasing charge (number not actual value)

64
Q

rank in order of increasing ionic size:

K+, S2-, Cl-

A

K+ < Cl- < S2-

65
Q

metallic radius

A

one half the shortest distance between nuclei of bonded atoms

66
Q

covalent radius

A

one half shortest distance between nuclei of adjacent individual atoms

67
Q

How does Zeff relate to atomic size

A

As Zeff increases atomic size decreases

68
Q

What is the periodic trend of atomic radius

A

across a period and up a period atomic radius decreases (biggest in bottom left, smallest in top right)

69
Q

What is the periodic trend of ionization energy

A

opposite of atomic radius, (biggest in top right, smallest in bottom left) (anomaly between N and O, and Be and B)

70
Q

what is the periodic trend of electron affinity

A

increases across a period and decreases down a group

71
Q

What are the 4 periodic trends about bonding

A

Zeff, IE, EA all increase up and across, while atomic radius is opposite

72
Q

What is the periodic trend of metallic behavior

A

metallic behavior decreases up and across

73
Q

what is the group 1 periodic trend of reactivity, and what agent is it

A

reactivity increases down group 1, good reducing agent

74
Q

What is the period trend of halogen reactivity, and what agent is it

A

halogen reactivity decreases down the group, good oxidizing agent

Chemistry 101 (1 decks)

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