Ch 5 Section 2 Flashcards

1
Q

Stability o noble gases results from

A

The gases special electron configurations

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2
Q

Generally the electron configurations of an atoms highest occupied energy level governs

A

The atoms chemical properties

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3
Q

Elements are arranged vertically in periodic table in groups that share

A

Similar chemical properties

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4
Q

Periods

A

Horizontal rows

7 in the modern periodic table

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5
Q

Length of each period is determined by the number of

A

Electrons that can occupy the sublevels being filled in that period

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6
Q

The 1s sublevel is being filled in the

A

First period

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7
Q

1s sublevel can hold a total of

A

2 electrons, and thus, it consists of two elements

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8
Q

In the second period the following sublevels are being filled

A

2s

2p

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9
Q

2s sublevel can hold

A

2 electrons

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10
Q

2p sublevel can hold

A

6 electrons

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11
Q

Second period totals

A

8 elements

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12
Q

Filling of the 3s and 3p sublevels accounts for

A

The eight elements of the third period

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13
Q

Filling 3d and 4d sublevels in addition to s and p sublevels adds

A

10 elements to both the fourth and fifth periods

Thus each of these periods totals 18 electrons

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14
Q

Filling 4f sublevels in addition to s p and d sublevels adds

A

14 elements to 6th period which totals 32 elements

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15
Q

As new elements are created the 25 named elements in period 7 could be

A

Extended to 32

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16
Q

Period of an element can be determined from the

A

Elements electron configuration

Coefficient in highest energy level= period

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17
Q

Periodic table is divided into

A
4 blocks
S
P
D
F
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18
Q

Elements of the s block are chemically

A

Reactive metals

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19
Q

Group 1 metals are more reactive than

A

Those of group 2

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20
Q

The ease with which the single electron is lost helps to make the group 1 metals

A

Extremely reactive

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21
Q

The elements of group 1 of the periodic table

A

(Lithium, sodium, potassium, rubidium, cesium, francium) known as the alkali metals

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22
Q

In pure state all alkali metals have a

A

Silvery appearance and are soft enough to cut with a knife

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23
Q

Alkali metals are not found in

A

Nature as free elements

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24
Q

Alkali metals combine

A

Vigorously with most nobmetals and react strongly with water to produce hydrogen gas and aqueous solutions of substances known as alkalis

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25
Alkali metals are usually stored in
Kerosene
26
Preceding down the volume the elements of group 1 melt at
Successively lower temperatures
27
The elements of group 2 of the periodic table
(Beryllium, magnesium, calcium, strontium, barium, radium) are called the alkaline earth metals
28
Atoms of alkaline-earth metals contain a
Pair of electrons in their outermost s sublevel
29
Group configuration for group 2 is
ns^2
30
Group configuration of group 1 is
ns^1
31
Group 2 metals are (comparison with alkali metals)
Harder Denser Stronger Higher melting pts than alkali metals
32
Alkaline earth metals are also too
Reactive to be found in nature as free elements
33
Hydrogen does not share the
Same properties as elements of group 1 | Unique element
34
Helium has ns^2 configuration like group 2 but is part of
Group 18
35
Because its highest occupied energy level is filled by two electrons helium possessed
Special chemical stability exhibiting the unreactive nature of a group 18 element
36
Group 2 metals have no
Special stability | Highest occupied energy levels aren't filled because each metal has an empty p sublevel
37
For energy level n there are
N possible sublevels
38
In addition to the two ns electrons of group 2 Atoms of the group 3 elements each have
One electron in the d sublevel of the (n-1) sublevel
39
Group configuration for group 3 is
(n-1)d^1ns^2
40
Atoms of the group 12 elements have
10 electrons in the d sublevel plus two electrons in the ns sublevel
41
Group configuration for group 12 is
(n-1)d^10ns^2
42
The d block elements are metals with
Typical metallic properties and are often referred to as transition elements
43
D block elements are
Good conductors of electricity and have a high luster | Typically Less reactive than alkali metals and alkaline earth metals
44
Some d block elements are so unreactive that they do not
Easily form compounds, existing in nature as free elements
45
Atoms of all p block elements contain
2 electrons in the ns sublevel
46
The p block elements together with the s block elements are called the
Main group elements
47
For group 13 elements added electron enters the
Np sublevel giving group configuration of ns^2np^1
48
Atoms of group 14 elements contain 2 electrons in p sublevel giving
ns^2np^2 for group configuration
49
Group configuration for 13-18
ns^2np^1-6
50
For atoms of p block elements the total number of electrons in the highest occupied level is equal to
The group number minus 10
51
At right hand end p block includes all of the
Nobmetals except hydrogen and helium
52
All six of the metallloids are also in the
P block
53
At the left hand side and bottom of the p block there are
Eight p block metals
54
The elements of group 17
(Fluorine, chlorine, bromine, iodine, astatine) | Are known as halogens
55
Halogens are the most reactive
Nonmetals
56
The reactivity of halogens is based on the presence of
7 electrons in their outer energy levels- one electron short of the stable noble gas configuration
57
Fluorine and chlorine are
Gases at room temp
58
Bromine is a
Reddish liquid
59
Iodine is a
Dark purple solid
60
Astatine is a synt
Synthetic element prepared in only very small quantities
61
Metallloids are located between
Nonmetals and metals in p block
62
Metals of the o block are generally
Harder and denser than the s block alkaline earth metals but softer and less dense than the d block metals
63
With exception of bismuth the metals of p block are sufficiently
Reactive to be found in nature only in form of compounds
64
The position of f block elements reflects the fact that
They involve the filling of the 4f sublevel
65
Lanthanides are shiny
Metals similar in reactivity to alkaline earth metals
66
Actinides are all
Radioactive | First four found naturally and remaining are lab made
67
Group 18 elements of the periodic table undergo
Few chemical reactions