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Chem 103 > Midterm 1 > Flashcards

Midterm 1 Flashcards

1
Q

What can matter be separated into

A

Pure substances and mixtures

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2
Q

What can pure substances be separated into

A

Elements and compounds

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3
Q

What can mixtures be separated into

A

Homogeneous and heterogeneous

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4
Q

What is the difference between elements and compounds

A

Elements are made of one type of atom and compounds are made of more than one type of atom

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5
Q

What are the five hypothesis’ of dalton’s atomic theory

A

1) matter is composed of extremely small particles called atoms

2) an element consists of only one type of atom

3) atoms of one element differ in properties from atoms of all other elements

4) a compound consists of atoms of two or more elements combined in a small, whole number ratio

5) atoms are neither created nor destroyed during a chemical change

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6
Q

What three laws did dalton’s atomic model account for

A

1)Law or conservation of matter

2) law of constant composition

3) law of multiple proportions (two elements can react to form more than one compound), carbon oxygen can form one thing or another thing

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7
Q

What did JJ Thompson show and through what experiment

A

The existence of electrons through the cathode ray tube

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8
Q

What were JJ Thompson’s 3 conclusions on electrons

A

1) negatively charged particles

2) less massive than atoms

3) particles were indistinguishable regardless of the source material (cathode ray)

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9
Q

What were the two things Millikan calculated in the oil drop experiment

A

1) charge of an electron

2) used Thomson’s charge to mass ratio to calculate the mass of an electron

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10
Q

What does Thomson’s plum pudding (raisin bun) model show

A

Electrons are dispersed in a cloud of positively charged matter

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11
Q

What is the modern representation of the atomic structure called

And what did it show

A

The nuclear atom

Showed that a positively charged mass is present in the atom and there was a lot of space

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12
Q

Atomic symbols: What does the left superscript show

A

Mass number

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13
Q

What is mass number

A

Number of protons + neutrons

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14
Q

Atomic symbols: what does a left subscript show

A

Atomic number

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15
Q

What is atomic number

A

=protons = electrons in a neutral atom

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16
Q

How to determine the number of neutrons in an atom

A

Mass #- atomic #

(Left superscript-left subscript)

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17
Q

What are isotopes

A

Atoms of the SAME element with the SAME # of protons but DIFF # of neutrons

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18
Q

What is atomic mass and where is it on the periodic table

A

An average # based on the amount of each isotope in nature

Located in the bottom of each element

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19
Q

Where is atomic number on the periodic table

A

Top left

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20
Q

What are ions

A

An atom or group of atoms that carry a net positive or negative charge

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21
Q

What is a cation and what is it’s charge

A

Formed when an atom LOSES electrons (+ charge)

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22
Q

What is an anion and what is it’s charged

A

Firmed when an atom GAINS electrons (- charged)

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23
Q

Why do ions form and when

A

Some atoms have a tendency to lose electrons and others have the tendency to gain electrons

Happens during chemical reactions

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24
Q

What is a column of elements called

And what do they have in common

A

Group

Have similar properties and reactivities

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25
Q

What is a row of elements called

A

Period

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26
Q

How are groups labeled

A

From left to right

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27
Q

How to figure out charge and when elements could have two charges

A

___\

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28
Q

Ionic compounds 1st group: , What are they formed from and what are they a combination of

And what element does what

A

Formed from monoatomic

Combination of metal and non metal because opposite charges attract

Metal loses electrons to form cation

Non metal gains electrons to form anion

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29
Q

Steps for naming ionic compounds

A

1) name cation

2) add “ide to name of the anion

3) specify charge of metals that form MORE than one ion in Roman numerals

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30
Q

What are monoatomic ions

A

____

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31
Q

What are polyatomic ions

A

____

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32
Q

Ionic compounds 2nd group: what are they combined of and what do they exist as

A

2 or more atoms that have been joined by covalent bonds

Exist as a charged unit

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33
Q

What are covalent bonds

A

____

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34
Q

How to name ionic compounds formed from polyatomic ions

A

____

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35
Q

Polyatomic ion: ammonium

(cation or anion)

A

NH4+

Cation

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36
Q

Polyatomic ion: hydronium

(cation or anion)

A

H3O+

Cation

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37
Q

Polyatomic ion: acetate

(cation or anion)

A

CH3COO-

or

C2H3O2-

Anion

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38
Q

Polyatomic ion: cyanide

(cation or anion)

A

CN-

Anion

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39
Q

Polyatomic ion: hydroxide

(cation or anion)

A

OH-

Cation

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40
Q

Polyatomic ion: hypochlorite

(cation or anion)

A

ClO-

Anion

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41
Q

Polyatomic ion: chlorite

(cation or anion)

A

ClO2-

Anion

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42
Q

Polyatomic ion: chlorate

(cation or anion)

A

ClO3-

Anion

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43
Q

Polyatomic ion: perchlorate

(cation or anion)

A

ClO4-

Anion

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44
Q

Polyatomic ion: nitrite

(cation or anion)

A

NO2-

Anion

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45
Q

Polyatomic ion: nitrate

(cation or anion)

A

NO3-

Anion

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46
Q

Polyatomic ion: permanganate

(cation or anion)

A

MnO4-

Anion

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47
Q

Polyatomic ion: carbonate

(cation or anion)

A

CO3(2)-

Anion

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48
Q

Polyatomic ion: hydrogen carbonate/ bicarbonate

(cation or anion)

A

HCO3-

Anion

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49
Q

Polyatomic ion: chromate

(cation or anion)

A

CrO4(2)-

Anion

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50
Q

Polyatomic ion: dichromate

(cation or anion)

A

Cr2O7(2)-

Dichromate

Anion

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51
Q

Polyatomic ion: peroxide

(cation or anion)

A

O2(2)-

Anion

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52
Q

Polyatomic ion: phosphate

(cation or anion)

A

PO4(3)-

Anion

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53
Q

Polyatomic ion: hydrogen phosphate

(cation or anion)

A

HPO4(2)-

Anion

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54
Q

Polyatomic ion: dihydrogen phosphate

(cation or anion)

A

H2PO4-

Anion

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55
Q

Polyatomic ion: sulfite

(cation or anion)

A

SO3(2)-

Anion

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56
Q

Polyatomic ion: sulfate

(cation or anion)

A

SO4(2)-

Anion

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57
Q

Polyatomic ion: hydrogen sulfate/ bisulfate

(cation or anion)

A

HSO4(2)-

Anion

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58
Q

What is the first type of covalent compounds and what are they a combination of

A

Binary compounds

Combination of non metal and non metal

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59
Q

How to name binary compounds

A

1) add “ide” to the end of second element

2) add numerical prefixes to both elements to indicate the subscript of each element

-don’t use mono for the first

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60
Q

What are the covalent compound prefixes in order

A

Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca

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61
Q

What is the second type of covalent compounds and what do they contain at least one of

(And why)

A

Acids

Contain at least one hydrogen atom

Because acids produce hydronium ions (H3O+) when dissolved in water

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62
Q

What are binary acids made of and how do you name

A

H bonded to another non metal or polyatomic ion

Naming
1) hydro_____ic acid

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63
Q

What are oxyacids made of and why

A

Contain H, O, and another non metal

Combination of oxygen and other non metal forms an oxoanion

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64
Q

How to name oxyacids

A

1) identify group

XO- : hypo_____ite

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65
Q

___

A

_

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66
Q

What are the 3 parameters that characterize a wave

A

Wavelength

Frequency

Speed

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67
Q

What is wavelength

A

Distance between two consecutive crests or troughs

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68
Q

What is frequency, and what variable is it

A

Number of complete cycles that pass a given point per second

v

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69
Q

What is speed (in waves), and what variable is it

A

Distance a wave propagates per unit time

s

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70
Q

What formula relates the 3 wave parameters and what is each measured in

A

s=v(wavelength)

s=m/s
v=Hz or s^-1
wavelength=nm

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71
Q

What is a wave

A

A vibration by which energy is transmitted

72
Q

As frequency increases, _____ decreases

A

Wavelength

73
Q

As wavelength increases, ______ decreases

A

Frequency

74
Q

What were Max Plancks two conclusions

A

1) energy can be emitted only in discrete energy packets rather than in a continuous wave

2) energy is quantized and it constitutes of small packets called quanta

75
Q

What is a quantum

A

The smallest amount of energy that can be absorbed or emitted in the form of electromagnetic radiation

76
Q

What formula describes the energy of a quantum

A

E=hv

77
Q

The change in an atoms energy occurs when the atom ____/_____ one or more quanta

And what formula describes this

A

Emits/absorbs

triangle E=nhv

Where n=1,2,3…

78
Q

What happened in the photoelectric effect

A

When a metal surface is exposed to light, electrons are ejected

79
Q

Three observations that are characteristics of the photoelectric effect

A

1) presence of a threshold frequency (V not)

2) intensity of light shine onto the metal surface

3) Frequency and Ek of the ejected electrons

80
Q

Photoelectric effect: no electrons leave the ____ of the metal ____ the threshold frequency, each metal has its own ______ _____

A

Surface

Below

Threshold frequency

81
Q

Photoelectric effect: an electron can only break free when it _____ enough energy to ____ its attraction to the ______

A

Absorbs

Breaks

Atom

82
Q

Photoelectric effect: increasing the ______ of the light shone on the metal surface above the _____ ____ DOESNT _____ the # of electrons ejected

A

Frequency

Threshold frequency

Increase

83
Q

Photoelectric effect: increasing the ____ of the light with frequency above the _____ ___ DOES ____ the # of electrons ejected

(And why)

A

Intensity

Threshold frequency

Increase

(Higher intensity light has more photons and each photon is used to free an electron)

84
Q

Photoelectric effect: increasing frequency of the incident light=____ Ek of the elected electrons

(And what type)

A

Increasing

(Linear)

85
Q

Photoelectric effect:
Formula that relates frequency and kinetic energy of the ejected electrons

(And what do all the v’s represent)

A

Ek=hv-hv(not) = (1/2)mv^2

1st: freq of incident light
2nd: threshold freq
3rd: velocity of electrons after ejected

86
Q

Ek=E-_____

E(not)=hv(not)=____

A

E(not)

Min amount of energy required to extract an electron

87
Q

Photoelectric effect: when question says “1 mole of photons” what do you have to do

A

Multiply final answer by avagadro’s number

88
Q

Atomic specta: elements give________ line spectra

A

Discontinuous

89
Q

What are the four quantum numbers and what variable do they go with

A

1) principal quantum #, n

2)angular momentum, l

3) magnetic quantum #, ml

4) electron spin quantum #, ms

90
Q

What is “n” and how do you find it

A

Defined the size and energy of the orbital

Find through periodic table

91
Q

As “n” gets bigger it means a bigger ____, which is also at higher ____, because it’s farther from the nucleus

A

Orbital

Energy

92
Q

What is “l” and how do you find it

A

Describes the shape (type) of orbital

Allowed values are from 0 to (n-1)

93
Q

What are the corresponding orbitals to the “l” value

A

l=0 s orbital
l=1 p orbital
l=2 d orbital

94
Q

What is “ml” and how do you find it

A

Refers to the 3D orientation of the orbital in the space surrounding the nucleus

ml= -l to +l

95
Q

What are the corresponding orbitals to the “ml” value and how many spaces do these orbitals have

A

ml=0 s orbital (only 1)

ml= -1,0,1 p orbital (3)

ml= -2,-1,0,1,2. d-orbital (5)

96
Q

What does the d orbital having 5 spaces mean

A

Set of 5 orbitals in 5 different orientations

97
Q

What is “ms” and how do you find it

A

Describes the orientation of the electron occupying the orbital

-1/2 down spin

1/2 up spin

98
Q

Electrons are orbiting the nucleus and also ____

a -1/2 parked with 1/2 ____ the atoms ability to produce its own _____ field

A

Spinning

Reduces

Magnetic

99
Q

Two electrons in an orbital CANNOT be characterized by the ____ set of quantum numbers

Every number can be the same EXPECT ___

A

Same

ms

100
Q

What are orbitals also called

A

Sub shells

101
Q

What is the ml value of the s orbital

What is the ml value of the p orbital

A

0

-1,0,1

102
Q

What is the l value of the s probital

What is the l value of the p orbital

What is the l value of the d orbital

A

0

1

2

103
Q

What is orbital notation

What are the 4 #’s for 3S

A

n(l) subscript (ml)

n=3
l= 0
ml=0
ms= -1/2 or 1/2

104
Q

Why doesn’t the 2d orbital exist

A

n=2

So l=0
l=1

There can only be s and p orbitals (cuz of l values)

105
Q

Pauli’s exclusion principle: a given orbital CANNOT contain two electrons with the same ___ because two electrons cannot have the same set of _____ _____

A

Spin

Quantum numbers

106
Q

What is a node

And what can they also be called

A

Regions where electrons can’t go

Spectral nodes or nodal spheres

107
Q

Formula for finding # of nodes in an orbital

How many nodes does 1S have? 3S?

A

of nodes =n-1

1S= no nodes

3S= 2 nodes

108
Q

Probability density is the highest _____ to the nucleus

(And why)

A

closest

(Small area/ given amount of electrons) = large density

So higher chance of finding an electron in a smaller area

109
Q

Stoich steps

A

1) write a balanced equation

2) calculate moles of 1st reactant
-con

Maybe add pic

110
Q

At the nucleus the radial probability distribution is ___

A

0

111
Q

In a radial probability distribution graph, everytime the line touches the x axis its a ____

A

Node

112
Q

What do Pz, Px, and Py orbital looks like

A

Pz= two flower petals OVER on z axis

Px= two flower petals OVER x axis

Py= two flower petals OVER y axis

113
Q

How do you indicate nodes in drawings

A

+ and - signs

114
Q

How many d orbitals are there, what are they, what planes are they orientated on

A

5

dyz = on y and x axis

dxz = on x and x axis

dxy = on x and y axis

dx^2-y^2 = oriented DIRECTLY on x and y axis

dz^2 = oriented DIRECTLY on z axis with ring in between

115
Q

How to draw d orbitals in 2 d

A

Switch labels of the two axis

116
Q

Where to draw flower petals for d orbitals

(And two exceptions)

A

BETWEEN the axis lines

dx^2-y^2
And
dz^2

Are oriented DIRECTLY on axis lines

117
Q

Example of a one electron atom

A

Hydrogen

118
Q

In a one electron atom, orbitals with the same ___ have the ____ energy

(What does this look like)

A

n

Same

3S, 3p, 3D orbital are all in line in the same level

119
Q

Degenerate

A

Have the same energy

120
Q

In a many electron atom orbitals with the same ___ have ___ energy

A

n

Different

121
Q

Many electron atoms: the ___ orbital is ____ penetrating than the p and d orbitals

A

s

more

122
Q

Many electron atom: does the 2p or 2s have more energy

A

2p

123
Q

Orbital penetration means that the orbital has ___ electron ____ closer to the nucleus

A

Higher

Density

124
Q

In a radial probability graph does the 2p or 2s reach its max first and why

A

2p max happens first

The electrons in the 2p spend more time closer to the nucleus because it has a smaller radius

125
Q

What is shielding

A

Electrons on an energy level closer to the nucleus shield energy levels further away from the nuclear attractive force

126
Q

More shielding= ____ penetrating=____ energy

A

More

Less

127
Q

Less shielding=___ penetrating= _____ energy

A

Less

Higher

128
Q

What is the order from most shielding to least shielding

A

s,p,d,f

129
Q

As the number of ____ increases and ofc number of electrons increases, the energy of the orbital goes ____

Protons are able to ___ electrons closer, so electrons get ___ to the nucleus and are ____ in energy

A

Protons

Down

Pull

Closer

Lower

130
Q

Greater nucleus charge ____ orbital energy

A

Lowers

131
Q

Electron electron repulsion _____ orbital energy because repulsion _____ the system

A

Increases

Stabilizes

132
Q

Electrons in outer orbitals are ___ shielded from the full nuclear charge so they have ____ energy

A

Shielded

Higher

133
Q

Orbitals with good penetration have ___ energy

A

Lower

134
Q

What is good penetration

A

Have electron density closer to the nucleus

135
Q

Formula for Zeff

(And what does inner shell mean)

A

of protons-inner shell electrons

Inner shell= all other shells except last occupied shell

136
Q

Force of attraction the outer electron will feel is determined by ______

A

Zeff

137
Q

Larger ___= outmost electrons are feeling ____ pull= makes atom ___

A

More

Smaller

138
Q

What does the superscript when writing electron configurations show

A

How many electrons are on that level

139
Q

What is paramagnetic

More unpaired electrons= _____ attraction to magnetic field

A

There’s at least one unpaired electron

Higher

140
Q

What is diamagnetic

And they are repelled by a ____ ___

A

No unpaired electrons

Magnetic field

141
Q

The Aufbau principle: when an atom or ion is in its ____ state, electrons fill the orbitals of the ____ available energy before occupying higher energy levels

A

Ground

Lowest

142
Q

Order for filling orbitals with electrons

A

1S, 2S, 2P, 3S, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6S, 4f, 5d, 6p, 5f, 6d, 5g, 6f, 6g, 6h

143
Q

How to figure out the number of VALENCE electrons in condensed electron configuration

A

All the subscripts added up

144
Q

How to figure out the number of INNER SHELL electrons in condensed electron configuration

A

All the electrons in the square brackets

145
Q

When ionizing you take the electrons from the ___ numbered shell

What she’ll wojld you take electrons from 3S or 4s

A

HIGHEST

4s

146
Q

Pg 40-43

A

___

147
Q

Elements are arranged in the periodic table in increasing ______ ____

A

Atomic number

148
Q

What are the three periodic table trends

A

-atomic size and ionic size

-ionization energy

-electron affinity

149
Q

Atomic size: in a group atomic size/atomic radius increases ____ a group

And why

A

Down

The # of electrons increases and the occupy a new shell, more shielding, size increases

150
Q

Which way does a period go for trends

A

Left to right

151
Q

Atomic size: in a period atomic size/atomic radius ____ across a period

And why

A

Decreases

Zeff increases and stronger nuclear attraction pulls electrons closer to the atom

152
Q

Metals lose valence ____ to form ____

Nonmetals gain valence ___ to form ___

A

Electrons

Cations

Electrons

Anions

153
Q

Oxidation numbers!!

A

___

154
Q

How to predict the “magnetic behaviour” of ions in a compound!!!

A

——

155
Q

Trends in ionic radii: ionic radius ____ down a group but ______ across a period

A

Increases

Decreases

156
Q

Trends in ionic radii: higher proton to electron ratio= ____ size

A

Smaller

157
Q

What is a high ratio!!!

A

__

158
Q

Is ionization endothermic or exothermic and why

A

Endothermic because it requires energy

159
Q

Does first ionization require more energy or 4th

And why

A

4th

since those electrons are closer to the nucleus

160
Q

Trends in ionization energy: ionization energy of elements _____ down a group

And why

A

of core electrons increases, so more shielding, so easier to remove outside electron

Decreases

161
Q

Trends in ionization energy: ionization energy of elements ____ across a period

And why

A

Increases

Zeff increases across a period

162
Q

Trends in ionization energy: Na has one valence electrons and Mg has 2, which has the higher 2nd ionization energy

And why

A

Na

Because it takes more energy to remove a core electron since with Mg there’s another valences electron to remove

163
Q

Trends in ionization energy: what is the first discontinuity

Why

How does this discontinuity extend

A

B has LOWER ionization energy than Be

B has three orbital levels while Be, only has two, so there’s more shielding is higher in B, easier to take an electron out

Extends vertically down those elements

164
Q

Trends in ionization energy: what is the second discontinuity

Why

How does this discontinuity extend

A

O has LOWER ionization energy than N

In the out shell of N all the electrons are unpaired, makes it the most stable, so more energy needed to remove electron, electron electron repulsion forces in outer shell of O makes electron easier to remove

Discontinuity extends vertically down

165
Q

Trends in electron affinity: it is the ___ change that occurs when an atom or ion in its ____ state ____ an electron

And what does it depend on

A

Energy

Gaseous

Gains

Depends on atomic size

166
Q

Is electron affinity endothermic or exothermic

and why

A

Exothermic

Cuz the nucleus must attract the electron strongly enough

167
Q

Trends in electron affinity: across a period EA ___

And why

A

Increases

Because atomic size decreases

168
Q

Trends in electron affinity: down a group EA ____

And why

A

Decreases

Because atomic size increases

169
Q

Is EA value positive or negative

A

Negative

170
Q

Larger EA (not including negative sign) = ____ for atom to accept the electron

A

Easier

171
Q

Oh 51-53!!!

A

___

172
Q

What are group 1 elements called

And what is their fundamental characteristic, so they are ____

A

Alkali metals

The ease with which they lose their valence electron, so very reactive

173
Q

Oxidation state of oxygen

A

-2

174
Q

Oxidation state of hydrogen

A

+1

175
Q

Oxidation state of group 2 metals (and where are they located)

A

+2

Second from the left

176
Q

Which is the oxidizing agent

A

The one being reduced

177
Q

What is the reducing agent

A

The one being oxidized

Chem 103 (13 decks)

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