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Chemistry 121 > Exam 2 blocks 4-6 > Flashcards

Exam 2 blocks 4-6 Flashcards

1
Q

What is the periodic table?

A

a graphical representation of all the known elements

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2
Q

What does periodic law state?

A

when elements are arranged according to increasing atomic number, elements having similar properties fall into place at regularly occurring intervals on the P table

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3
Q

Where are you most likely to find an element with similar properties?

A

the same vertical column

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4
Q

What are the periods on the periodic table?

A

the horizontal rows on the table numbered 1-7

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5
Q

What element numbers are the lanthanides?

A

58-71

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6
Q

What element numbers are the actinides?

A

90-103

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7
Q

What are lanthanides and actinides collectively called?

A

inter transition elements

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8
Q

What are the vertical columns on the periodic table?

A

groups labled IA-VIIIA

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9
Q

All but what group are known as representitive elements?

A

VIIIA

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10
Q

All elements accept H in group IA are called?

A

Alkali metals

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11
Q

What is the name of group IIA?

A

Alkaline Earth Metals

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12
Q

What are the elements in group VIIA?

A

Halogens

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13
Q

What are the elements in group VIIIA?

A

Noble Gasses.

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14
Q

What is group B referred to?

A

transition elements

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15
Q

How many metaloids are there?

A

8

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16
Q

What are noble elements?

A

Elements that are unreactive and usually found in an uncombined state

Au,Ag, Pd, Pt, Ta

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17
Q

What are the most unreactive of all of the elements?

A

The noble gasses

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18
Q

How many elements are solid at room temp?

A

104

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19
Q

What are the two types of solids?

A

Crystalline

Amorphous

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20
Q

What is a crystalline solid?

A

solids that have Very predictable, repeating, densely packed structures

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21
Q

What two elements are liquid at room temp?

A

Bromine and Mercury

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22
Q

Which noble gas is the most dense?

A

Xe Xenon

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23
Q

How many elements are gasses at room temp?

A

11

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24
Q

Minimum energy equals ____?

A

maximum stability

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25
Principal energy levels are also called?
Shells
26
What are the three divisions of shells
shells subshells orbitals
27
What is a shell?
A region of space containing electrons that spend most of their time approx. the same distance from the nucleus and have similar energies
28
What is the maximum number of electrons that any shell can hold?
2n^2
29
The maximum number of subshells within a shell is the same as?
the shell number
30
What are the four letters in order assigned to subshells?
S P D F
31
How many electrons can a S shell hold at max?
2
32
How many electrons can a P shell hold at max?
6
33
How many electrons can a D shell hold at max?
10
34
How many electrons can a F shell hold at max?
14
35
How many electrons at max can be in an orbital?
2
36
How many orbitals does an S shell have?
1
37
How many orbitals does an P shell have?
3
38
How many orbitals does an D shell have?
5
39
How many orbitals does an F shell have?
7
40
What does it mean for an electron to be degenerate?
It has the same energy level as the other electrons within the same subshell
41
What does the pauli exclusion principal state?
that electrons in the same orbital must have opposite spins
42
What are the two parts of hunds rule?
1) All orbitals in the same subshell will get one electron before any electrons are paired in an orbital 2) Unpaired electrons in the same subshell will all have the same spin
43
What are the two types of chemical compounds?
Ionic compounds | Molecular Compound
44
What are ionic compounds composed of?
Formula units
45
What are formula units composed of?
Ions
46
What is another work for molecular compounds?
covalent
47
What are molecular compounds composed of?
molecules
48
What are molecules composed of?
charge neutral atoms
49
What is a chemical bond?
The attractive force that chemically bonds atoms or ions into complex units
50
What are the two types of chemical bonds?
Ionic and covalent
51
What does ionic bonding require?
a transfer of electrons
52
What happens to a charge if electrons are lost?
it becomes positive
53
What happens to a charge if electrons are gained?
it becomes negative
54
What is a cation?
a positively charged ion
55
What is an anion?
a negatively charged ion
56
WHat are the two conditions for an ionic bond?
the charges must be opposite and of the same magnitude
57
Why do ions form?
The quest for an octet of valence electrons and greater stability
58
What is electronegativity?
the numerical measure of the attractive force an atom has for electrons
59
Define formula unit
The smallest whole-number repeating ratio of ions present in an ionic compound that results in charge nutrality
60
Which is bigger, a cation or an anion? why
An anion is bigger because it gains electrons to become an anion. more electrons = higher volume
61
Ions ___ elections | Molecules___electrons
Transfer | Share
62
How many electrons to form one covalent bond?
2 | 1 pair
63
What increases electron density?
When electrons are localized
64
High electron density = ?
High strength
65
What is a molecular orbital?
A unique orbit formed when tow atomic orbits come together
66
What is hybridization?
The process in which two atomic orbits overlap and form a new molecular orbit
67
What are two ways the strength of a covalent bond can be increased?
Decreasing the area in which the electrons are localized placing more electrons into the same area forming multiple bonds
68
How many electrons are involved per bond?
2
69
What are lone pair electrons?
valence electrons not involved in a bond
70
what are bonding electrons?
electrons involved in a bonding pair
71
What bond shares electrons?
Covalent
72
What bond transfers electrons?
ionic
73
Which type of bond involves all valence electrons?
ionic
74
Which type of bond forms between similar atoms?
covalent
75
Which type of bond forms between dissimilar atoms?
ionic
76
What compounds are formed from formula units?
Ionic
77
What compounds are formed from molecules?
Covalent
78
What bond can form multiple bonds?
covalent
79
What bond can only for single bonds?
Ionic
80
IN which bond do bonded electrons hybridize?
covalent
81
In what instances are the electrons in a covalent molecular orbital shared equally?
Homoatomic Diatomic elements
82
What causes the unequal sharing of electrons in covalent bonds?
slight variations in the electronegativity
83
Which side of a polar covalent bond is negative
the side with the highest electronegativity
84
Are polar molecules charged?
no. The negative and positive charges are both of equal intensity and cancel each other out
85
Which bonds have a large difference in electronegativity?
ionic
86
Which bonds have small differences in electronegativity?
polar covalent
87
Which bonds have no difference in electronegativity?
non-polar covalent bonds
88
If the difference in electronegativity is zero then the bond is?
non-polar covalent
89
If the difference in electronegativity is between zero and 1.5, then the bond is?
polar covalent
90
If the difference in electronegativity is greater than 2, the bond is
Ionic
91
If the difference in electronegativity is between 1.5 and 2 and there is no metal in the bond then the bond is?
polar-covalent
92
If the difference in electronegativity is between 1.5 and 2 and there is metal in the bond then the bond is?
Ionic
93
As bond strength increases the bond take son more ___ characteristics
Ionic
94
What causes Molecular polarity?
The presence of polar bonds and the way they are arranged in the molecule
95
When is a molecule non-polar?
if the molecule has no polar bonds or if the polar bonds in the molecule are arranged in a way that the polar charges cancel each other out
96
What does the Pauli exclusion principle state?
Electrons in the same orbital must have opposite spins
97
What are the two parts to Hunds rule?
1-all orbitals within the same su shell will get one electron before any electrons are paired in an orbital 2-unpaired electrons in the same subshell will have the same spin
98
What does the octet rule state?
When forming ions, atoms lose or gain e- in such a way so that their e- configuration will match the noble gas closest to them in the periodic table

Chemistry 121 (6 decks)

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