Ch 4 Section 3 Flashcards

1
Q

The arrangement of electrons in an atom is known as the atoms

A

Electron configuration.

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2
Q

Because atoms of different elements have different numbers of electrons a unique

A

Electron configuration exists for the atoms of each element

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3
Q

Like all systems in nature electrons in atoms tend to

A

Assume arrangements that have the lowest possible energies

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4
Q

The lowest energy arrangement of the electrons for each element is called they

A

Elements ground state electron configuration

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5
Q

To build up electron configurations for the ground state of any particular atom

A

First the energy levels of the orbitals are determined

Then electrons are added to orbitals one by one according to three basic rules

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6
Q

According to the aufbau principle an electron occupied the

A

Lowest energy orbital that can receive it

Shows the order in which electrons occupy orbitals

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7
Q

Beginning with the third main energy level n = 3, the energies of sublevels in different main energy levels

A

Begin to overlap

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8
Q

The 4s sublevel is lower in energy to the

A

3d sublevel

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9
Q

4s sublevel is filled before an electrons

A

Enter the 3d orbitals

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10
Q

Less energy is required for two electrons to pair up in the 4s orbital than for

A

Those two electrons to occupy a 3d orbital

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11
Q

The second rule reflects

A

Importance of spin quantum number

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12
Q

According to the Pauli exclusion principle no two electrons in the same atom can

A

Have the same set of four quantum numbers

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13
Q

The two values of he spin quantum number reflect the fact that for

A

2 electrons to occupy the same orbital they must have opposite spin states

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14
Q

Third rule requires placing as many

A

Unpaired electrons as possible in separate orbitals in the same sublevel

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15
Q

In this way electron electron repulsion is

A

Minimized so that the electron arrangements have the lowest energy possible

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16
Q

According to hunds rule orbitals of equal energy are each occupied by one electron before any orbital he

A

Occupied by a second electron and all electrons in singly occupied orbitals must have the same spin state

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17
Q

Applying hunds rule shows that one electron will enter each of the three

A

P orbitals in a main energy level before a second electron entered any of them

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18
Q

3 methods or notations are used to indicate

A

Electron configurations

Third notation is mostly used with elements of the third period and higher

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19
Q

(Orbital notation) an unoccupied orbital is represented by a

A

Line with the orbitals name written underneath the line

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20
Q

(Orbital notation) the lines are labeled with the

A
Principal quantum number and sublevel letter. 
Ex: orbital notation for helium 
He ⬆️⬇️
      -------
       1s
21
Q

Electron configuration notation eliminated the

A

Lines and arrows of orbital notation

22
Q

(Electron configuration notation) instead the number of k

Electrons in a sublevel is shown by

A

Adding a superscript to the sublevel designation

23
Q

In the first period elements (hydrogen and helium) electrons occupy

A

The orbital of the first main energy level

24
Q

According to the aufbau principle after the 1s orbital is filled the next electron occupies the

A

S sublevel in the second main energy level

25
The highest occupied energy level is the electron containing main energy level with the
Highest principal quantum number
26
Inner she'll electrons are electrons that are not in the
Highest occupied energy level
27
According to the aufbau principle the next electron must pair with another electron in one of the
2p orbitals as long as the spins of the paired electrons are opposite
28
Atoms such as those of neon which have the s and p sublevels of their highest occupied level filled with eight electrons are said to
Have an octet of electrons
29
After the outer octet is filled in neon the next electron enters the
S sublevel in the n= 3 main energy level
30
The first 10 electrons in an atom of each of the third period elements have the
Same configuration as neon which allows us to use a shorthand notation for the configurations
31
(Noble gas notation) the group 18 elements are called
Noble gases
32
(Noble gas notation) to simplify notation of third period elements the symbol for neon is
Enclosed j square brackets and the rest of the configuration follows
33
A noble gas configuration refers to an outer main energy level occupied
In most cases by eight electrons
34
The fourth period begins by filling the
4s orbital, the empty orbital of lowest energy
35
With the 4s sublevel filled the
4p and 3d sublevels sre the next available vacant orbitals
36
The 3d sublevel is lower in energy than the
4p sublevel. Therefore the five 3d orbitals are next to be filled
37
A total of 10 electrons can occupy the
3d orbitals
38
Fourth period element configurations begin with
[Ar]
39
According to hunds rule one electron is added to each of the three
4p orbitals before electrons are paired in any 4p orbital
40
In the 18 elements of the fifth period sublevels fill in a similar manner as in
Elements of the fourth period but start at the 5s orbital instead of the 4s
41
Successive electrons are added to the first to the 5s orbital then to the
4d orbitals and finally to the 5p orbitals
42
The sixth period consists of
32 elements
43
To build up electron configurations for the sixth period electrons are added first to the
6s orbital in cesium and barium. Then jn lanthanum an electron is added to the 5d orbital
44
With cerium 4f orbitals
Begin to fill
45
Next 5d orbitals are filled and the period is completed by filling the
6p orbitals
46
Because the 4f and 5d orbitals are very close in energy number our deviations from the simple rules
Occur as these orbitals are filled
47
The seventh period is
Incomplete and consists largely of synthetic elements
48
The quantum model of the atom improves on the Bohr model because it
Describes the arrangements of electrons in atoms other than hydrogen