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Chemistry I > Chapter 7 & 8 > Flashcards

Chapter 7 & 8 Flashcards

1
Q

Enables us to label completely an electron in any orbital in any atom

A

The Four Quantum Numbers (n , l , mₗ , mₛ)

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2
Q

What are the Address of an electron in an atom

A

The four quantum numbers

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3
Q

Atoms

A

Is The smallest unit of matter that can’t be broken down chemically

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4
Q

Can an atom be broken down ?

A

Yes, an atom can be broken down, but not chemically

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5
Q

Proton

A

A positively charged charged subatomic particle

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6
Q

Electron

A

A Negatively charged charged subatomic particle

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7
Q

Neutron

A

A subatomic particle with no Charge

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8
Q

Atomic mass (A) =

A

protons + neutrons

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9
Q

Atomic Number (Z) =

A

of Protons or Electrons

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10
Q

The four quantum numbers

A

Shorthand

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11
Q

The four quantum numbers

A

Describes the charistarics of electrons position

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12
Q

The four quantum numbers

A

predicts an electron behavior

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13
Q

n

A

Principal quantum number

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14
Q

Principal quantum number ( n )

A

All orbitals with the same n are in the same shell

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15
Q

Principal quantum number ( n )

A

describes the energy level of an e-

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16
Q

l

A

Secondary quantum number

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17
Q

Secondary quantum number

A

describes the shape orbital where e- is found

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18
Q

Secondary quantum number

A

Divides shells into smaller groups called subshells

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19
Q

mₗ

A

magnetic quantum number

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20
Q

magnetic quantum number

A

divides shells into individual orbitals

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21
Q

mₛ

A

Magnetic spin quantum number

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22
Q

Magnetic spin quantum number

A

describes the angular momentum of an electron (e- spin)

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23
Q

only takes positive integer values

A

n

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24
Q

increasing n increases the ..

A

Size of an orbital

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25
increasing n increases the ..
total energy of an orbital
26
number of nodes increases by increasing
n
27
distance between an electron an its nucleus depends on
n
28
RHhc =
1.7x10^-18 J/Atom
29
Orbital angular momentum Quantum number
l
30
specifies orbital angular momentum of e-
l
31
angular variation of e- path
l
32
kinetic energy of orbital
l
33
potential energy of orbital
n
34
Magnetic quantum number
ml
35
Allowed values for Magnetic QN
(-l , 0 , +l)
36
there are 2l+1 different values for
ml
37
z axis component of orbital angular momentum or how much angular momentum is aligned to a axis
ml
38
determines orintation of orbital in space
ml
39
to designate specific orbital you need
3 QN
40
to designate specific orbital you need
(n , l , ml)
41
Spin Quantum Number
ms
42
arises out of behaviour of e in megnatic feild
ms
43
e- acts like a top
ms
44
leads to 2 possible directions of e spin
ms
45
Electron Configureation
Is how the electrons are distributed among various atomic orbitals
46
any atom with an odd number of electrons will
always contain one or more unpaired spins
47
any atom with an odd number of electrons is
paramagnetic
48
any atom with an odd number of electrons is
unpaired
49
atoms containing an even number of electrons
may or may not contain unpaired spins.
50
Aufbau principle
dictates that as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to the atomic orbitals.
51
What does A stand for
Atomic Mass
52
What does Z Stand fopr
Atomic Number
53
Early version of the periodic table
Arranged by increasing atomic mass ( A )
54
Early version of the periodic table
made by mendeleev (Russian) & meyer (German) in 1869
55
Early version of the periodic table
noted repeating (Periodic ) properties
56
Modern periodic table
Arranged by increasing atomic number ( Z )
57
Modern periodic table
Rows called periods
58
Modern periodic table
Columns called groups or families
59
Modern periodic table
1 - 18 standard international
60
1A Group is called
Alkali metals (Except H)
61
1A Group is called
Alkali metals
62
2A Group is called
Alkaline earth metals
63
7A Group is called
halogens
64
8A Group is called
Nobel gases
65
4f
lanthanides
66
5f
actinides
67
Very Reactive metals
Alkali metals 1A
68
Tends to form +1 Ions
Alkali metals 1A
69
Reacts with oxygen
Alkali metals 1A
70
Forms a compound that dissolves in water
Alkali metals 1A
71
Yield strongly caustic or alkaline solution (M2O)
Alkali metals 1A
72
Alkaline earth metals
2A
73
Reactive
Alkaline earth metals
74
Tends to form +2 ions
Alkaline earth metals
75
Oxygen compounds are strongly alkaline (MO)
Alkaline earth metals
76
Many are not water soluble
Alkaline earth metals
77
Found in deposits in the ground
Alkaline earth metals
78
Halogens
Derived from the greek word meaning sea or salt
79
Halogens are in the
7A
80
Reactive
Halogens
81
Form Diatomic molecules in elemental state
Halogens
82
Forms -1 ions with alkali metals-----Salts
Halogens
83
Noble gases
8A
84
inert----very unreactive
noble gases
85
Only heavier elemtns of group react & then very limited
Halogens
86
Don't form charged ions
Halogens
87
Monatomic gases
Halogens
88
Representative / Main group elements are
halogens
89
Representative / Main group elements are
alkaline earth metals
90
Representative / Main group elements are
alkali metals
91
B group
ends with d
92
All are metals
B group elements
93
begins in 4th row
B group elements
94
tends to form ions with several different charges
B group elements
95
lanthanide elements
They are elements from 58-71
96
Actinide elements
elements 90 - 103
97
At bottom of periodic table
actinide elements
98
tends to form +2 and +3 ions
actinide elements
99
Radioactive elements
Actinide
100
on the left side of the periodic table
metals
101
upper right hand corner
Non metals
102
diagnol line between metals & nonmetals
mettaloids
103
Cations
positive charged ions formed from metals Atoms lose electrons
104
Anions
Negative charged ions Formed from non metals atoms gain electron
105

Chemistry I (1 decks)

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