Midterm 1 Flashcards

(177 cards)

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
What is a row of elements called
Period
26
How are groups labeled
From left to right
27
How to figure out charge and when elements could have two charges
___\
28
Ionic compounds 1st group: , What are they formed from and what are they a combination of And what element does what
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
29
Steps for naming ionic compounds
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
30
What are monoatomic ions
____
31
What are polyatomic ions
____
32
Ionic compounds 2nd group: what are they combined of and what do they exist as
2 or more atoms that have been joined by covalent bonds Exist as a charged unit
33
What are covalent bonds
____
34
How to name ionic compounds formed from polyatomic ions
____
35
Polyatomic ion: ammonium (cation or anion)
NH4+ Cation
36
Polyatomic ion: hydronium (cation or anion)
H3O+ Cation
37
Polyatomic ion: acetate (cation or anion)
CH3COO- or C2H3O2- Anion
38
Polyatomic ion: cyanide (cation or anion)
CN- Anion
39
Polyatomic ion: hydroxide (cation or anion)
OH- Cation
40
Polyatomic ion: hypochlorite (cation or anion)
ClO- Anion
41
Polyatomic ion: chlorite (cation or anion)
ClO2- Anion
42
Polyatomic ion: chlorate (cation or anion)
ClO3- Anion
43
Polyatomic ion: perchlorate (cation or anion)
ClO4- Anion
44
Polyatomic ion: nitrite (cation or anion)
NO2- Anion
45
Polyatomic ion: nitrate (cation or anion)
NO3- Anion
46
Polyatomic ion: permanganate (cation or anion)
MnO4- Anion
47
Polyatomic ion: carbonate (cation or anion)
CO3(2)- Anion
48
Polyatomic ion: hydrogen carbonate/ bicarbonate (cation or anion)
HCO3- Anion
49
Polyatomic ion: chromate (cation or anion)
CrO4(2)- Anion
50
Polyatomic ion: dichromate (cation or anion)
Cr2O7(2)- Dichromate Anion
51
Polyatomic ion: peroxide (cation or anion)
O2(2)- Anion
52
Polyatomic ion: phosphate (cation or anion)
PO4(3)- Anion
53
Polyatomic ion: hydrogen phosphate (cation or anion)
HPO4(2)- Anion
54
Polyatomic ion: dihydrogen phosphate (cation or anion)
H2PO4- Anion
55
Polyatomic ion: sulfite (cation or anion)
SO3(2)- Anion
56
Polyatomic ion: sulfate (cation or anion)
SO4(2)- Anion
57
Polyatomic ion: hydrogen sulfate/ bisulfate (cation or anion)
HSO4(2)- Anion
58
What is the first type of covalent compounds and what are they a combination of
Binary compounds Combination of non metal and non metal
59
How to name binary compounds
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
60
What are the covalent compound prefixes in order
Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca
61
What is the second type of covalent compounds and what do they contain at least one of (And why)
Acids Contain at least one hydrogen atom Because acids produce hydronium ions (H3O+) when dissolved in water
62
What are binary acids made of and how do you name
H bonded to another non metal or polyatomic ion Naming 1) hydro_____ic acid
63
What are oxyacids made of and why
Contain H, O, and another non metal Combination of oxygen and other non metal forms an oxoanion
64
How to name oxyacids
1) identify group XO- : hypo_____ite
65
___
_
66
What are the 3 parameters that characterize a wave
Wavelength Frequency Speed
67
What is wavelength
Distance between two consecutive crests or troughs
68
What is frequency, and what variable is it
Number of complete cycles that pass a given point per second v
69
What is speed (in waves), and what variable is it
Distance a wave propagates per unit time s
70
What formula relates the 3 wave parameters and what is each measured in
s=v(wavelength) s=m/s v=Hz or s^-1 wavelength=nm
71
What is a wave
A vibration by which energy is transmitted
72
As frequency increases, _____ decreases
Wavelength
73
As wavelength increases, ______ decreases
Frequency
74
What were Max Plancks two conclusions
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
What is a quantum
The smallest amount of energy that can be absorbed or emitted in the form of electromagnetic radiation
76
What formula describes the energy of a quantum
E=hv
77
The change in an atoms energy occurs when the atom ____/_____ one or more quanta And what formula describes this
Emits/absorbs triangle E=nhv Where n=1,2,3…
78
What happened in the photoelectric effect
When a metal surface is exposed to light, electrons are ejected
79
Three observations that are characteristics of the photoelectric effect
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
Photoelectric effect: no electrons leave the ____ of the metal ____ the threshold frequency, each metal has its own ______ _____
Surface Below Threshold frequency
81
Photoelectric effect: an electron can only break free when it _____ enough energy to ____ its attraction to the ______
Absorbs Breaks Atom
82
Photoelectric effect: increasing the ______ of the light shone on the metal surface above the _____ ____ DOESNT _____ the # of electrons ejected
Frequency Threshold frequency Increase
83
Photoelectric effect: increasing the ____ of the light with frequency above the _____ ___ DOES ____ the # of electrons ejected (And why)
Intensity Threshold frequency Increase (Higher intensity light has more photons and each photon is used to free an electron)
84
Photoelectric effect: increasing frequency of the incident light=____ Ek of the elected electrons (And what type)
Increasing (Linear)
85
Photoelectric effect: Formula that relates frequency and kinetic energy of the ejected electrons (And what do all the v’s represent)
Ek=hv-hv(not) = (1/2)mv^2 1st: freq of incident light 2nd: threshold freq 3rd: velocity of electrons after ejected
86
Ek=E-_____ E(not)=hv(not)=____
E(not) Min amount of energy required to extract an electron
87
Photoelectric effect: when question says “1 mole of photons” what do you have to do
Multiply final answer by avagadro’s number
88
Atomic specta: elements give________ line spectra
Discontinuous
89
What are the four quantum numbers and what variable do they go with
1) principal quantum #, n 2)angular momentum, l 3) magnetic quantum #, ml 4) electron spin quantum #, ms
90
What is “n” and how do you find it
Defined the size and energy of the orbital Find through periodic table
91
As “n” gets bigger it means a bigger ____, which is also at higher ____, because it’s farther from the nucleus
Orbital Energy
92
What is “l” and how do you find it
Describes the shape (type) of orbital Allowed values are from 0 to (n-1)
93
What are the corresponding orbitals to the “l” value
l=0 s orbital l=1 p orbital l=2 d orbital
94
What is “ml” and how do you find it
Refers to the 3D orientation of the orbital in the space surrounding the nucleus ml= -l to +l
95
What are the corresponding orbitals to the “ml” value and how many spaces do these orbitals have
ml=0 s orbital (only 1) ml= -1,0,1 p orbital (3) ml= -2,-1,0,1,2. d-orbital (5)
96
What does the d orbital having 5 spaces mean
Set of 5 orbitals in 5 different orientations
97
What is “ms” and how do you find it
Describes the orientation of the electron occupying the orbital -1/2 down spin 1/2 up spin
98
Electrons are orbiting the nucleus and also ____ a -1/2 parked with 1/2 ____ the atoms ability to produce its own _____ field
Spinning Reduces Magnetic
99
Two electrons in an orbital CANNOT be characterized by the ____ set of quantum numbers Every number can be the same EXPECT ___
Same ms
100
What are orbitals also called
Sub shells
101
What is the ml value of the s orbital What is the ml value of the p orbital
0 -1,0,1
102
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
0 1 2
103
What is orbital notation What are the 4 #’s for 3S
n(l) subscript (ml) n=3 l= 0 ml=0 ms= -1/2 or 1/2
104
Why doesn’t the 2d orbital exist
n=2 So l=0 l=1 There can only be s and p orbitals (cuz of l values)
105
Pauli’s exclusion principle: a given orbital CANNOT contain two electrons with the same ___ because two electrons cannot have the same set of _____ _____
Spin Quantum numbers
106
What is a node And what can they also be called
Regions where electrons can’t go Spectral nodes or nodal spheres
107
Formula for finding # of nodes in an orbital How many nodes does 1S have? 3S?
# of nodes =n-1 1S= no nodes 3S= 2 nodes
108
Probability density is the highest _____ to the nucleus (And why)
closest (Small area/ given amount of electrons) = large density So higher chance of finding an electron in a smaller area
109
Stoich steps
1) write a balanced equation 2) calculate moles of 1st reactant -con Maybe add pic
110
At the nucleus the radial probability distribution is ___
0
111
In a radial probability distribution graph, everytime the line touches the x axis its a ____
Node
112
What do Pz, Px, and Py orbital looks like
Pz= two flower petals OVER on z axis Px= two flower petals OVER x axis Py= two flower petals OVER y axis
113
How do you indicate nodes in drawings
+ and - signs
114
How many d orbitals are there, what are they, what planes are they orientated on
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
How to draw d orbitals in 2 d
Switch labels of the two axis
116
Where to draw flower petals for d orbitals (And two exceptions)
BETWEEN the axis lines dx^2-y^2 And dz^2 Are oriented DIRECTLY on axis lines
117
Example of a one electron atom
Hydrogen
118
In a one electron atom, orbitals with the same ___ have the ____ energy (What does this look like)
n Same 3S, 3p, 3D orbital are all in line in the same level
119
Degenerate
Have the same energy
120
In a many electron atom orbitals with the same ___ have ___ energy
n Different
121
Many electron atoms: the ___ orbital is ____ penetrating than the p and d orbitals
s more
122
Many electron atom: does the 2p or 2s have more energy
2p
123
Orbital penetration means that the orbital has ___ electron ____ closer to the nucleus
Higher Density
124
In a radial probability graph does the 2p or 2s reach its max first and why
2p max happens first The electrons in the 2p spend more time closer to the nucleus because it has a smaller radius
125
What is shielding
Electrons on an energy level closer to the nucleus shield energy levels further away from the nuclear attractive force
126
More shielding= ____ penetrating=____ energy
More Less
127
Less shielding=___ penetrating= _____ energy
Less Higher
128
What is the order from most shielding to least shielding
s,p,d,f
129
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
Protons Down Pull Closer Lower
130
Greater nucleus charge ____ orbital energy
Lowers
131
Electron electron repulsion _____ orbital energy because repulsion _____ the system
Increases Stabilizes
132
Electrons in outer orbitals are ___ shielded from the full nuclear charge so they have ____ energy
Shielded Higher
133
Orbitals with good penetration have ___ energy
Lower
134
What is good penetration
Have electron density closer to the nucleus
135
Formula for Zeff (And what does inner shell mean)
# of protons-inner shell electrons Inner shell= all other shells except last occupied shell
136
Force of attraction the outer electron will feel is determined by ______
Zeff
137
Larger ___= outmost electrons are feeling ____ pull= makes atom ___
More Smaller
138
What does the superscript when writing electron configurations show
How many electrons are on that level
139
What is paramagnetic More unpaired electrons= _____ attraction to magnetic field
There’s at least one unpaired electron Higher
140
What is diamagnetic And they are repelled by a ____ ___
No unpaired electrons Magnetic field
141
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
Ground Lowest
142
Order for filling orbitals with electrons
1S, 2S, 2P, 3S, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6S, 4f, 5d, 6p, 5f, 6d, 5g, 6f, 6g, 6h
143
How to figure out the number of VALENCE electrons in condensed electron configuration
All the subscripts added up
144
How to figure out the number of INNER SHELL electrons in condensed electron configuration
All the electrons in the square brackets
145
When ionizing you take the electrons from the ___ numbered shell What she’ll wojld you take electrons from 3S or 4s
HIGHEST 4s
146
Pg 40-43
___
147
Elements are arranged in the periodic table in increasing ______ ____
Atomic number
148
What are the three periodic table trends
-atomic size and ionic size -ionization energy -electron affinity
149
Atomic size: in a group atomic size/atomic radius increases ____ a group And why
Down The # of electrons increases and the occupy a new shell, more shielding, size increases
150
Which way does a period go for trends
Left to right
151
Atomic size: in a period atomic size/atomic radius ____ across a period And why
Decreases Zeff increases and stronger nuclear attraction pulls electrons closer to the atom
152
Metals lose valence ____ to form ____ Nonmetals gain valence ___ to form ___
Electrons Cations Electrons Anions
153
Oxidation numbers!!
___
154
How to predict the “magnetic behaviour” of ions in a compound!!!
——
155
Trends in ionic radii: ionic radius ____ down a group but ______ across a period
Increases Decreases
156
Trends in ionic radii: higher proton to electron ratio= ____ size
Smaller
157
What is a high ratio!!!
__
158
Is ionization endothermic or exothermic and why
Endothermic because it requires energy
159
Does first ionization require more energy or 4th And why
4th since those electrons are closer to the nucleus
160
Trends in ionization energy: ionization energy of elements _____ down a group And why
Decreases # of core electrons increases, so more shielding, so easier to remove outside electron
161
Trends in ionization energy: ionization energy of elements ____ across a period And why
Increases Zeff increases across a period
162
Trends in ionization energy: Na has one valence electrons and Mg has 2, which has the higher 2nd ionization energy And why
Na Because it takes more energy to remove a core electron since with Mg there’s another valences electron to remove
163
Trends in ionization energy: what is the first discontinuity Why How does this discontinuity extend
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
Trends in ionization energy: what is the second discontinuity Why How does this discontinuity extend
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
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
Energy Gaseous Gains Depends on atomic size
166
Is electron affinity endothermic or exothermic and why
Exothermic Cuz the nucleus must attract the electron strongly enough
167
Trends in electron affinity: across a period EA ___ And why
Increases Because atomic size decreases
168
Trends in electron affinity: down a group EA ____ And why
Decreases Because atomic size increases
169
Is EA value positive or negative
Negative
170
Larger EA (not including negative sign) = ____ for atom to accept the electron
Easier
171
Oh 51-53!!!
___
172
What are group 1 elements called And what is their fundamental characteristic, so they are ____
Alkali metals The ease with which they lose their valence electron, so very reactive
173
Oxidation state of oxygen
-2
174
Oxidation state of hydrogen
+1
175
Oxidation state of group 2 metals (and where are they located)
+2 Second from the left
176
Which is the oxidizing agent
The one being reduced
177
What is the reducing agent
The one being oxidized