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AS Chemistry > 2.2.1 - Electron Structure > Flashcards

2.2.1 - Electron Structure Flashcards

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1
Q

What is the equation to work out how many electrons can go in each shell?

A

2n^2, where n is the principle quantum number.

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2
Q

How many electrons in the 1st shell?

A

2

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3
Q

How many electrons in the 2nd shell?

A

8

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4
Q

How many electrons in the 3rd shell?

A

18

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5
Q

How many electrons in the 4th shell?

A

32

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6
Q

What are atomic orbitals?

A

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

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7
Q

How many electrons can each orbital hold?

A

2

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8
Q

What shape are S orbitals?

A

Spherical

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9
Q

What shape are P orbitals?

A

Dumbbells.

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10
Q

How many P orbitals in a shell?

A

3

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11
Q

How many orbitals in an S shell?

A

1

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12
Q

How many orbitals in a P shell?

A

3

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13
Q

How many orbitals in a D shell?

A

5

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14
Q

How many orbitals in an F shell?

A

7

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15
Q

Why don’t electrons in orbitals repel each other?

A

Because of a property called spin. The two electrons have opposite spin.

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16
Q

What is electronic configuration?

A

The arrangement of electrons in an atom or ion.

17
Q

When building up an atom which shells are filled up first?

A

The atom with the lowest available energy.

18
Q

How is a subs hell built up?

A

Each orbital is filled singly before pairing starts.

19
Q

Why does 4s orbital fill before the 3d?

A

It has a slightly lower energy level.

20
Q

What is the electronic configuration of Li (atomic number 3)?

A

1s2, 2s1

21
Q

What is the electronic configuration of Li+?

A

1s2.

22
Q

Electronic configuration of copper? Just last shells.

A

4s2 3d10

23
Q

Electronic configuration of chromium? Last shells only.

A

4s2 3d5

24
Q

What is the first ionisation energy?

A

Energy required to remove one mole of electrons from one mole of gaseous atoms producing ions of charge 1+.

25
Q

Why don’t orbitals repel each other?

A

Because of a property called spin.

AS Chemistry (24 decks)

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