Unit 2 Key Terms Flashcards
(169 cards)
1
Q
Law of Conservation (of matter)
A
mass (or matter) is not created or destroyed in chemical reactions.The total mass of all products equals the total mass of all reactants
2
Q
Law of Constant Composition (Law of Definite
Proportions)
A
compounds consist of elements combined
in definite proportions by mass.
3
Q
Points which Dalton’s Atomic Theory were wrong
A
1) Atoms can be divided - they consist of smaller particles
called protons, neutrons, and electrons (subatomic
particles).
2) Atoms of the same element can have different masses
(isotopes).
4
Q
What are the 3 subatomic particles and their charges
A
Protons-Positive(+)
Neutrons-Neutral
Electrons-Negative(-)
5
Q
What was the first subatomic particle discovered?
A
The Electron
6
Q
Proton Mass
A
1.6726 x 10-24 g or 1.007 amu
7
Q
Neutron Mass
A
1.6749 x 10-24 g or 1.008 amu
8
Q
Electron Mass
A
9.109 x 10-28 g or 0.000549 amu
9
Q
Equal to the number of Protons in the nucleus
A
Electrons
10
Q
Like charges ___ and Unlike charges ___
A
Repel;Attract
11
Q
1 amu=
A
1.6605387 x 10-24 g
12
Q
An atom is electrically _____
A
Neutral: Protons=electrons
13
Q
Mass Number
A
Protons+Neutrons= Mass Number
14
Q
If an atom (or isotope) of oxygen contains 8
protons, 10 neutrons, and 8 electrons, what is its
1) atomic number, 2) net charge, 3) mass number?
A
1) 8 (Oxygen) (O)
2) Neutral
3) 18
15
Q
Atoms of the same element that have different mass numbers
A
Isotopes
16
Q
How many protons are in any zinc atom?
A
30
17
Q
How many neutrons are in a zinc atom with a
mass number of 65?
A
35
18
Q
What is the mass number of a different zinc
isotope that has 37 neutrons in its nucleus?
A
67
19
Q
In an atomic or isotopic symbol. the mass number is the ___ and the atomic number is the ____
A
superscript;subscript
20
Q
Ions are formed when
A
- form when atoms lose or gain electrons.
- have unequal numbers of protons and electrons.
- have a net electrical charge.
21
Q
Groups of bonded atoms with a net
charge are called
A
polyatomic ions
22
Q
Ions derived from single atoms are called
A
Monatomic Ions
23
Q
Positive Ions
A
Cations
24
Q
Negative Ions
A
Anions
25
A + in superscript on an Ion is representative of
electrons lost
26
A - in superscript on an ion is representative of
electrons gained
27
Metal ions have the same name as
the parent atom
| Na-Sodium Na+ Sodium Ion
28
Atoms of nonmetals can gain electrons to reach an octet, forming
monatomic ions
29
Monatomic anions are named by taking the root of the
| element name and adding
```
-ide
O = oxygen atom F = fluorine atom
O2− = oxide ion F− = fluoride ion
N = nitrogen atom Br = bromine atom
N3− = nitride ion Br− = bromide ion
```
30
Ionic compounds
• contain a combination of cations and anions in
charge balance (i.e. is neutral).
• have attractions called ionic bonds between
cations and anions.
• have high melting and boiling points.
• are solid at room temperature.
31
To name ionic compounds, give the name of the
| _____then the name of the _____
Cation;Anion
NaCl = sodium chloride
32
CaCl2
Calcium Chloride
33
Li3N
Lithium Nitride
34
Al2O3
Aluminum Oxide
35
FeCl3
Iron (III) Chloride
36
Iron (II) Chloride
FeCl2
37
CuS
Copper Sulfide
38
a group of atoms with an overall net ionic charge. The atoms are bonded together by shared valence electrons, forming a distinct chemical unit.
Polyatomic Ion
39
NH4^+
Ammonium
40
NO3^-
Nitrate
41
CO3^ 2-
Carbonate
42
hydrogen carbonate
| bicarbonate
HCO3^ -
43
hydroxide
OH^−
44
nitrite
NO2^ -
45
phosphate
PO4 ^3−
46
Ca3(PO4)^2
Tricalcium Phosphate
47
LiNO3
Lithium Nitrate
48
Cu2SO3
Copper (I) Sulfite
49
Table Salt
Sodium Chloride (NaCl)
50
Bleach
Sodium Hypochlorite (NaClO)
51
Baking Soda
Sodium Bicarbonate (NaHCO3)
52
Electrons distributed in a cloud
Electron configuration of the atom
53
The speed of light
λ⋅ν = c (the speed of light)
54
c = 2.9979 x 108 m/s
The speed of light
55
Light with a ______ wavelength will have a___ frequency.
short; high
56
Light with a____wavelength will have a ____ frequency.
long; low
57
1 Angstrom Å
1 x 10^-10 m
58
Planck's constant
6.626 x 10-34 Js
59
Each element produces a unique line spectrum, or
spectral fingerprint
60
DeBroglie Equation:
λ =h/mv
wave-particle duality
61
Heisenberg Uncertainty Principle
- It is impossible to
know the position and energy (momentum) of electron
simultaneously.
62
quantum mechanics
a branch of physics that deals with light and
subatomic particles that exhibit wave-particle duality:The DeBroglie equation, the Heisenberg Uncertainty Principle, and the Schrödinger wave tequation
63
describe the size, energy, shape,
| and orientation of orbitals.
quantum numbers
64
the quantum number
| most directly related to the size. It has possible values of 1, 2, 3, 4, etc.
Principal Quantum Number (n)
65
The principal quantum number is associated with ___ of electrons. (Ex: An electron with an n = 3 is in the third
____.)
shell(s)
66
also
known as the secondary quantum number or azimuthal
quantum number, is the quantum number related to the shape of the orbital’s electron density map (electron cloud). It has a range of possible values of 0 up to n-1.
Examples: If n = 1, then l can only be 0.
If n = 4, then l could be 0, 1, 2, or 3
angular momentum quantum number (l)
67
The value of l is associated with a _____- a set of
| orbitals within a shell that have the same shape (or same value of l).
subshell
68
when l=0,
the orbital has a spherical shape centered around the nucleus.
69
What type of orbital is in every shell?
s orbital
70
When l=1
the electron density map of the orbital shows
| two distinct lobes, forming a “dumbbell” shape.
71
p orbitals
dumb-bell shape
72
When l=2
the probability density map gets more
| complicated. These orbitals are designated as d orbitals.
73
When l=3
the orbital shapes get even more complex.
| These orbitals are designated as f orbitals.
74
```
value of l:
0
1
2
3
have what orbital letter designation
```
s
p
d
f
75
Magnetic Quantum Number (ml)
is related to how an orbital is aligned in 3-dimensional space. The value of ml ranges from -l to l.
76
When l=0, m can only be
0. This means there is only one orientation for an s orbital.
77
When l = 1, ml can have values of
-1, 0, or 1. Each value corresponds to a different alignment for a p orbital.
78
There are ___ p orbitals in each p subshell.
3
79
When l = 2, ml can have values of
-2, -1, 0, 1 or 2. Each
| value corresponds to a different alignment for a d orbital.
80
There are____ d orbitals in each d subshell.
5
81
When l = 3, ml can have values of
-3, -2, -1, 0, 1, 2, or 3. Each value corresponds to a different alignment for an f orbital.
82
There are ____ f orbitals in each f subshell
7
83
Value of l: 0 1 2 3 subshell designation and # of orbitals within the subshell
a. n = 3, l = 1, ml = 0
b. n = 5, l = 3, ml = -2
s p d f
| 1 3 5 7
84
A set of quantum numbers that have the correct
| relationships among them
an “allowed set” of quantum
85
Pauli exclusion principle
says that no two electrons
in an atom can have the same values for all four quantum numbers.
This means that no more than two electrons can occupy one orbital.
Electron A: n = 3, l = 1, ml = 1, ms = +1/2
Electron B: n = 3, l = 1, ml = 1, ms = -1/2
86
In the second shell, two kinds of orbitals are possible
s and p
87
Because there are __ values for ml when l = 1, there are___ p orbitals of equal energy in the second shell.
3
88
Because there is only one value for ml
for an _ orbital, just
one s orbital is possible in the second shell. This will be
designated 2_
s
89
Aufbau Principle
Electrons in a ground state atom go into the lowest energy orbitals available
90
1s->2s->2p->3s->3p->4s->3d->4p
Subshell filling order
91
Hund's Rule
Electrons in orbitals of equal energy (i.e. within a subshell) spread out in separate orbitals and have parallel spins.
92
Valence Shell
is the highest numbered, outermost shell (highest value for n)
93
Electrons in the valence shell are called
Valence Electrons
94
What type of electrons are most important in chemistry and why?
Valence electrons are the most important for
chemistry - they can be lost or shared. Electrons
can sometimes be added to the valence shell.
95
core electrons.
Electrons below the valence shell, which do not normally participate in chemical reactions.
96
Core notation
starts with square brackets around
the last noble gas before the element followed by
a list of all the subshells and the number of
electrons in the subshells beyond the noble gas
core.
ex:Fe (Z = 26)
[Ar] 4s^2 3d^6
97
The number of shells in an atom is equal to
The row number
98
Configuration for Copper (Cu)
[Ar]4s^1 3d^10
99
[Ar]4s^1 3d^5
Configuration for Chromine(Cr)
100
Octet Rule
Because the ns^2p^6 configuration is very stable,
atoms tend to lose, gain, or share valence
electrons in order to be left with or to reach
that ns^2p^6 configuration.
2 + 6 = 8 = an octet
101
Elements that follow the duet rule instead of the octet rule
H, He, Li, and Be
102
Metals tend to ___ electrons
lose
103
nonmetals tend to ___ electrons
gain
104
Metals lose electrons from the _____ first.
highest numbered shell
105
Electrons are added to the _____ of a
| nonmetal.
valence shell
106
ionization energy (IE)
the energy required to
| remove an electron from a gas phase atom.
107
Ionization can be represented as:
X(g) + energy → X+(g) + e−
108
electron affinity (EA)
the energy change occurring when
| an electron is added to a gas phase atom
109
X(g) + e− → X−(g) + energy
Electron affinity can be represented as
110
metals and bigger atoms
- lower ionization energies
| lower electron affinities
111
nonmetals and smaller atoms
- higher ionization energies
| higher electron affinities
112
metallic character
The tendency of an element to display the chemical
| and physical properties of metals is known at
113
The trend for metallic character is exactly ____
| the trend for IE and EA.
opposite (down and left)
114
IE and EA generally increase in the directions indicated by the arrows.
right and up
115
Atomic size (radius) follows the same pattern as metallic character -
it increases down and to the left on the periodic table.
116
The size of an atom is determined by two things:
1) the number or shells of electrons
2) the effective nuclear charge (Zeff
) acting on the valence
electrons
117
Core electrons shield the charge of some of the ___ in the nucleus from the valence electrons. The valence electrons will be attracted to the leftover or “effective” nuclear charge (Zeff) outside the core.
Protons
118
Core electrons shield the charge of some of the ___ in the nucleus from the valence electrons. The valence electrons will be attracted to the leftover or “effective” nuclear charge (Zeff) outside the core.
Protons
119
When Zeff is greater, valence electrons are ______ more tightly, making a smaller electron cloud and giving the atom a higher electron affinity and higher ionization potential.
pulled in
120
When metals lose electrons, they lose ___
An entire shell
121
For transition metals that can also lose electrons
from _____, the more electrons that are lost,
the smaller the cation.
Therefore in terms of size: Fe > Fe2+ > Fe3+
d subshell
122
When nonmetals gain electrons, the _____
among the more crowded valence electrons
increase the size of the shell.
Repulsions
123
Cations are ___ than their parent atom
smaller
124
Anions are _____ than their parent atom
larger
125
Isoelectronic series –
– a set of ions and atoms that all have
the same number of electrons (and therefore the same
electron configuration)
126
The general trend for an isoelectronic series is:
The higher the atomic number, the smaller the ion or atom is
127
The general trend for an isoelectronic series is:
The higher the atomic number, the smaller the ion or atom is
128
ammonium permanganate
NH4MnO4
129
magnesium acetate
Mg(C2H3O2)2
130
strontium sulfate
SrSO4
131
Cu(OH)2
copper(II) hydroxide
132
strontium sulfide
SrS
133
copper(I) cyanide
CuCN
134
strontium sulfite
strontium sulfite
135
iron(II) oxide
FeO
136
potassium dichromate
K2Cr2O7
137
ammonium monohydrogen phosphate
(NH4)2HPO4
138
calcium bromide
CaBr2
139
mercury(II) periodate
Hg(IO4)2
140
NaHCO3
sodium bicarbonate
141
Na3PO4
sodium phosphate
142
Al2(CO3)3
aluminum carbonate
143
barium perchlorate
Ba(ClO4)2
144
Pb(NO3)2
lead(II) nitrate
145
magnesium chloride
MgCl2
146
CrP
chromium(III) phosphide
147
Fe2(SO3)3
iron(III) sulfite
148
NaClO
bleach
149
manganese(III) dihydrogen phosphate
Mn(H2PO4)3
150
lead(IV) dichromate
Pb(Cr2O7)2
151
Al(OH)3
Al(OH)3
152
Zn3(PO4)2
zinc phosphate
153
Na2S
sodium sulfide
154
Na2SO4
sodium sulfate
155
cobalt(II) hypochlorite
Co(ClO)2
156
Wavelength
The distance between two adjacent peaks
157
Frequency
The number of complete wavelengths or cycles that pass a given point each second
158
λ
wavelength (lambda)
159
c
speed of light
160
ν
(Nu)= frequency
161
Frequency equation
c=λν
162
Quantum
smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation
163
Planck's constant (h)
6.626*10^-34 Joule seconds
164
Momentum equation
mass*velocity
165
X-ray diffraction
When x-rays pass through a crystal, an interference pattern resilts that is characteristic of wave-like properties of EMR (Electron microscope and Micrograph)
166
What orbital type are transition metals
d
167
What orbital type are lanthanides and actinides
f
168
What orbital type are the right side of the table?
p
169
What orbital type are the left side of the table?
s
