Electronic configurations and the Periodic table Flashcards Preview

CfE Advanced Higher Chemistry Unit 1 > Electronic configurations and the Periodic table > Flashcards

Flashcards in Electronic configurations and the Periodic table Deck (19)
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1

What is the Aufbau principle?

Orbitals are filled in order of increasing energy. 1s before 2s

2

What is the order of orbital filling from 1s to 4d?

1s 2s 2p 3s 3p 4s 3d 4p 4d

3

What is the Pauli exclusion principle?

This states that an orbital cannot contain more than two electrons and they must have opposite spins.

4

What is Hund's rule of maximum multiplicity?

Electrons fill each degenerate orbital singly with spins parallel before pairing occurs.

5

What are the 2 types of notation used to represent the electron configurations of elements?

Spectroscopic notation and orbital box notation

6

What the spectroscopic notation for a lithium atom?

1s2 2s1

7

Which element has atoms with [Ar]4s1?

Potassium

8

How many electrons are there in the 2p sub-shell of the oxygen atom?

4

9

Which number would complete this spectroscopic notation for a nitrogen atom?

1s2 2s2 2p?

1s2 2s2 2p3

10

Carbon has two unpaired electrons. How many unpaired electrons would boron have?

1

11

What is the spectroscopic notation of a lithium ion?

1s2

12

Which element does this orbital box notation represent?

Hydrogen

13

Which element does this orbital box notation represent?

Fluorine

14

How would lithium be represented as orbital box notation?

15

How would oxygen be represented as orbital box notation?

16

Which areas represent elements which have s, p, d or f electrons in the outermost sub-shell?

17

1. Which element group appears at the four peaks?

2. Would the ionisation be easy or difficult?

3. Are these elements reactive or unreactive?

4. How many electrons in the outer shell?

1. These are group 0, noble gases.

2. Difficult as it is a high value.

3. Unreactive noble gases.

4. All are full, usually with 8 electrons

18

Why is there a slight dip in first ionisation energy from beryllium to boron?

Beryllium is 1s2 2s2 and boron is 1s2 2s2 2p1

Beryllium has a full sub-shell and is more stable. Boron has a single 2p electron and is less stable.

19

Why is there a dip  in first ionisation energy in the middle of the p-block from nitrogen to oxygen?

Nitrogen is 1s2 2s2 2p3 and oxygen is 1s2 2s2 2p4

Half filled sub-shells are relatively stable and it is easier to remove the fourth 'p' electron from the 2p shell of oxygen.