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Chemistry 101 > Unit 2 > Flashcards

Unit 2 Flashcards

(97 cards)

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1
Q

pure substances

A

ionic and moleculer

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2
Q

composed of two or more different atoms which have chemically combined

A

ionic and molecular

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3
Q

whole number ratios of atoms (represented by chemical formula)

A

ionic and molecular

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4
Q

when elements chemically combine electrons are lost by the metals to form cations and electrons are gained by the nonmetals to form anions

A

ionic compounds

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5
Q

when electrons chemically combine electrons are shared between atoms of nonmetals and/or metalloids

A

molecular

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6
Q

ions are not connected together to form a single unit. ions are held together by the attraction of opposite charges

A

ionic

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7
Q

atoms are connected together by the shared electrons to form a larger unit called a molecule

A

molecular

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8
Q

notice: no metals, ions or charges

A

molecular

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9
Q

when we write ions by themselves we must indicate the charge

A

ionic

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10
Q

amount of positive charge must balance the amount of negative charge in an ionic compound

A

ionic compound

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11
Q

7 diatomic elements

A 
Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine
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12
Q

the second energy level contains how many sublevels

A

two

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13
Q

the first energy level contains how many sublevels

A

one

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14
Q

the fourth energy level contains how many sub levels

A

four

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15
Q

the fifth energy level contains how many sub levels

A

five

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16
Q

the third energy level contains how many sub levels

A

three

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17
Q

a P sublevel has how many orbitals

A

three

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18
Q

P sublevel has a maximum capacity of how many electrons

A

six

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19
Q

a S sublevel has how many orbitals

A

one

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20
Q

S sublevel has a maximum capacity of how many electrons

A

two

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21
Q

a F sublevel has how many orbitals

A

seven

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22
Q

F sublevel has a maximum capacity of how many electrons

A

14

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23
Q

D sublevel has how many orbitals

A

five

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24
Q

D sublevel has a maximum capacity of how many electrons

A

10

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25
4th energy level would contain how many electrons when completely filled
32
26
5th energy level would contain how many electrons when completely filled
50
27
3RD energy level would contain how many electrons when completely filled
18
28
2ND energy level would contain how many electrons when completely filled
8
29
1ST energy level would contain how many electrons when completely filled
2
30
how many orbitals are present in the 3rd energy level
9
31
how many orbitals are present in the 1st energy level
1
32
how many orbitals are present in the 2nd energy level
4
33
5th energy level contains how many orbitals
(# of energy level squared) 5^2= 25
34
4th energy level contains how many orbitals
(# of energy level squared) 4^2=16
35
the maximum number of electrons that can be found in the highest energy level of any atom is
8
36
maximum number of electrons that can be found in a single D orbital is
2
37
maximum number of electrons that can be found in a single S orbital is
2
38
maximum number of electrons that can be found in a single P orbital is
2
39
those elements whose atoms have a stable electron configuration are members of group
8
40
the volume in space where we are most likely to find an electron is an
orbital
41
approx mass of protons
1 amu
42
approx mass of neutrons
1 amu
43
approx mass of electrons
- 1/1830 amu
44
what is the formula formed by Bohr for the radius of an electron
r=n2a0
45
how many electrons in the 4th energy level
32e- (2n^2)
46
how many electrons in the 2nd energy level
8e- (2n^2)
47
how many electrons in the 3rd energy level
18e- (2n^2)
48
how many electrons in the 1st energy level
2e- (2n^2)
49
viewed e- as slow moving particle moving around the nucleus
bohr
50
helped to explain emission spectra
bohr
51
e- moves very fast and behaves like light
quantum mechanical model
52
when it loses an electron it becomes
a cation
53
when it gains an electron it becomes
an anion
54
a region in space where we are most likely to find an electron
quantum mechanical model
55
e- in the outermost energy level
valence electrons
56
e- that are not in the outermost energy level
core electrons
57
known for their lack of reactivity
noble gases
58
T or F noble gases are stable. they have nothing to gain by reacting
true
59
all atoms want 8 valence electrons
octet rule
60
all atoms want 8 valence electrons except
Helium (2 valence e-)
61
n in quantum numbers represents
the energy level
62
L in quantum numbers represents
the sub level
63
equation for finding L
(n-1)
64
mL in quantum numbers represents
orbital
65
Ms in quantum numbers represents
electrons (arrows)
66
no two electrons in an atom can have the same set of quantum numbers
pauli exclusion principle
67
in orbital box diagrams each individual box represents WHAT and the entire ensemble represents WHAT
ORBITALS; SUBLEVEL
68
each orbital of a sublevel must contain an electron before pairing can begin
hund's rule
69
how atoms interact to form molecules and compounds
chemical bonding
70
write the symbol for the atom and then put dots around it to represent the number of valence electrons
lewis dot symbols
71
transfer of one (or more) e- from a metal to a nonmetal to form cations and anions with noble gas electron configuration
ionic bonding
72
pair of e- shared between two atoms
covalent bonding
73
using a diffraction grating plus a source of white light, we see a
continuous spectrum
74
all energies of light are being emitted
continuous spectrum
75
using a diffraction grating and a sample of Hydrogen with high voltage electricity is passed, we see
line spectrum
76
only a few energies of light are emitted
line spectrum
77
Each element has it's own unique
line spectrum
78
only way to separate a covalent bond is a
chemical change
79
who said that electrons in orbit
bohr
80
who said there were energy levels
bohr
81
maximum number of electrons= 2n^2
bohr
82
sublevels - s,p,d,f,g,h,i
quantum mechanical model
83
sublevels composed of orbitals
quantum mechanical model
84
energies of a sub level (or order of filling)
Aufbau principle
85
three methods of writing - spectroscopic notation, orbital box diagrams, quantum numbers
electron configuration
86
electron(s) are transferred from metal to nonmetal
Ionic Bonding
87
ions are not attached to one another
Ionic Bonding
88
full charges
Ionic Bonding
89
ionic bond – the force of attraction between oppositely charged ions
Ionic Bonding
90
sharing electrons – two nonmetals or metalloid & nonmetal
Covalent Bonding
91
atoms are connected by covalent bond – molecule
Covalent Bonding
92
Seven diatomic elements
Covalent Bonding
93
metal and nonmetal
ionic bond
94
two nonmetals
covalent bond
95
s orbitals are
spherical
96
p orbitals are
figure 8
97
d orbitals are
4 clover leaf, 5th looks like double sided pacifier

Chemistry 101 (8 decks)

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