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A level Chemistry > Chapter 5 - Electrons and Bonding > Flashcards

Chapter 5 - Electrons and Bonding Flashcards

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1
Q

How does group number relate to electronic structure?

A

The group number tells you how many electrons in the outermost shell.

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2
Q

What is a shell?

A

Shells are energy levels, the energy levels increase as the shell number increases. The shell number may also be referred to as principal quantum number.

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3
Q

What is an orbital?

A

A region around the nucleus that can hold up to two electrons with opposite spins.
It shows us a 95% probability of where an electron will exist.

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4
Q

How many electrons can shell 1 hold?

A

2 electrons

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5
Q

How many electrons can shell 2 hold?

A

8 electrons

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6
Q

How many electrons can shell 3 hold?

A

18 electrons

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7
Q

How many electrons can shell 4 hold?

A

32 electrons

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8
Q

What shape is an s-orbital?

A

A spherical shape

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9
Q

What shape is a p-orbital?

A

A dumb-bell shape

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10
Q

What is an electron?

A

A cloud of negative charge, which has the shape of the orbital occupied by the electron.

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11
Q

Which orbitals are in shell 1?

A

1 s-orbital

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12
Q

Which orbitals are in shell 2?

A

1 s-orbital and 3 p-orbitals

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13
Q

Which orbitals are in shell 3?

A

1 s-orbital, 3 p-orbitals and 5 d-orbitals.

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14
Q

Which orbitals are in shell 4?

A

1 s-orbital, 3 p-orbitals, 5 d-orbitals and 7 f-orbitals

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15
Q

What is a sub-shell?

A

All of the orbitals of the same type in the same shell.
e.g. s sub-shell and p sub-shells

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16
Q

How many electrons can an s sub-shell hold?

A

2 electrons

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17
Q

How many electrons can a p sub-shell hold?

A

6 electrons

18
Q

How many electrons can a d sub-shell hold?

A

10 electrons

19
Q

How many electrons can a f sub-shell hold?

A

14 electrons

20
Q

Order the sub-shells in terms of energy levels, starting from lowest.

A

s, p, d and f going up the shells.
With the exception of the 3d sub-shell which has a higher energy than 4s.

21
Q

Which sub-shells are in shell 1?

A

1s

22
Q

Which sub-shells are in shell 2?

A

2s, 2p

23
Q

Which sub-shells are in shell 3?

A

3s, 3p, 3d

24
Q

Which sub-shells are in shell 4?

A

4s, 4p, 4d, 4f

25
Q

What is the short notation for electronic structure?

A

The closest prior noble gas in square brackets and the remaining electronic configuration.

26
Q

How are orbitals drawn?

A

A square with two arrows in it pointing opposite directions to represent the opposite spins

27
Q

How are orbitals filled for ions?

A

Draw out the electronic structure of the atom.
For a negative ion, add the extra electrons.
For a positive ion, remove the electrons, if 4s is full remove the electrons from there before removing from 3d.

28
Q

What is the electronic structure of Chromium (Cr)?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5
As it is more stable due to both 4s and 3d being half-full.

29
Q

What is the electronic structure of Copper (Cu)?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10
As is makes a full 3d sub-shell and a half-full 4s sub-shell.

30
Q

What is ionic bonding?

A

Electrostatic attraction between positive and negative ions

31
Q

What are some common cations?

A

Metal ions and ammonium ions

32
Q

What are some common anions?

A

Non-metal ions and polyatomic ions

33
Q

What is the structure of ionic compounds?

A

Each ions attracts oppositely charged ions in all directions
Forms giant ionic lattices

34
Q

What are the properties of ionic compounds?

A

Almost all are solid at RTP
High melting and boiling points
Good conductors in liquid or aqueous form
Usually soluble

35
Q

What is a covalent bond?

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

36
Q

What two molecules is a covalent bond between?

A

Metal and non-metal

37
Q

Describe a single covalent bond.

A

A single shared pair of electrons from both the bonding atoms

38
Q

Describe multiple covalent bonding.

A

Multiple pairs of shared electrons from both the bonding atoms

39
Q

Describe a dative covalent bond.

A

A covalent bond where bond the electrons come from one of the bonding atoms only.

40
Q

What is average bond enthalpy?

A

Measurement of covalent bond strength.

A level Chemistry (29 decks)

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