2.2.1: Electron structure Flashcards

1
Q

What does the principal quantum number indicate?

A

The shell occupied by the electrons

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2
Q

What is a shell?

A

A group of orbitals with the same principal quantum number

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3
Q

How many electrons can the 3rd shell hold?

A

18

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4
Q

How many electrons can the 4th shell hold?

A

32

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5
Q

What is an orbital?

A

A region around the nucleus that can hold up to two electrons with opposite spins

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6
Q

How many electrons can an orbital hold?

A

2

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7
Q

What are the 4 types of orbitals

A

● s orbital
● p orbital
● d orbital
● f orbital

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8
Q

`What is the shape of a s-orbital?

A

Spherical

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9
Q

What is the shape of a p-orbital?

A

dumbbell shape

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10
Q

How many orbitals are found in a S subshell?

A

1

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11
Q

How many electrons can be held in a S subshell?

A

2

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12
Q

How many orbitals does P subshell have?

A

3

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13
Q

How many electrons can be held in a P subshell?

A

6

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14
Q

How many orbitals are present in a D subshell?

A

5

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15
Q

How many electrons can be held in a d-sub shell?

A

10

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16
Q

How many orbitals are found in a F subshell?

A

7

17
Q

How many electrons can fill F subshell?

A

14

18
Q

From which shell onwards is S orbital present?

A

n=1

19
Q

From which shell onwards is P orbital present?

A

n=2

20
Q

From which shell onwards is D orbital present?

A

n=3

21
Q

From which shell onwards is F orbital present?

A

n=4

22
Q

What are the rules by which electrons are arranged in a shell? (5 marks)

A

● Electrons are added one at a time
● Lowest available energy level is filled first
● Each energy level must be filled before the next one can fill
● Each orbital is filled singly before pairing
● 4s is filled before 3d

23
Q

Why does 4s orbital fill before 3d orbital?

A

4s orbital has a lower energy than 3d before it is filled

24
Q

What is the electron configuration of krypton?

A
1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p6
25
Q

Which electrons are lost when an atom becomes a positive ion?

A

Electrons in the highest energy levels