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Chemistry > Chapter 5 - Electrons and Bonding > Flashcards

Chapter 5 - Electrons and Bonding Flashcards

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1
Q

What are shells regarded as?

A

Energy levels

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2
Q

What happens to the energy level as the number of shells increase?

A

Energy increases

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3
Q

What is the shell number referred to as?

A

Principal quantum number

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4
Q

What are shells made up of?

A

Atomic orbitals

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5
Q

How many electrons can be held in an orbital?

A

One or two, but no more

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6
Q

How many orbitals does each letter (s, p, d, f) contain?

A

S - 1
P - 3
D - 5
F - 7

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7
Q

How many electrons can be held in each orbital type?

A

S - 2
P - 6
D - 10
F - 14

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8
Q

What is the shape of an s-orbital?

A

Spherical

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9
Q

What is the shape of a p-orbital?

A

Dumbbell

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10
Q

What are the rules of filling orbitals?

A

They fill in order of increasing energy
Orbitals with the same energy are occupied singly first, and then pair up with opposite spins. (meaning one arrow up and one arrow down).

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11
Q

Explain where the rule causes confusion for 3d and 4s.

A

The 4s sub-shell has lower energy than 3d, so the 4s fills before the 3d.
When the 4s fills up it takes higher energy level than 3d, so the 4s loses electrons first.

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12
Q

Explain the rule of electrons pair with opposite spins.

A

Electrons are negatively charged so they repel each other.
Electrons have spin up or spin down properties
So electrons pair up with opposite spin so that charge repulsion is counteracted and both electrons can be in same orbital.

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13
Q

How can electron figuration be shortened?

A

Write the previous noble gas plus leftover electrons.

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14
Q

What happens when forming ions in terms of energy sub-shells?

A

Highest energy sub-shells lose or gain electrons.

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15
Q

What is ionic bonding?

A

The electrostatic attraction between opposite charged ions.

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16
Q

What forms when ions attract oppositely charged ions in all directions?

A

Giant ionic lattice

17
Q

How are melting and boiling points of ionic compounds explained?

A

High temperatures are required to provide energy sufficient to overcome the strong electrostatic attraction between the ions.

18
Q

What happens to the melting point of giant ionic lattices when ionic charge increases?

A

Melting point increases as there is stronger attraction between ions.

19
Q

Are ionic compounds soluble?

A

Some are soluble in polar solvents like water because water molecules break down lattice and surround ions.

Some are not soluble because they have high charges so it is harder for water to break the ionic lattice.

20
Q

What does solubility require?

A

Ionic lattice must be broken down

Polar solvent must attract and surround each ion.

21
Q

What does solubility of ionic compounds depend on?

A

The strength of the attractions within the giant ionic lattice.
The attractions between ions and water molecules.

22
Q

When can ionic compounds conduct electricity?

A

They cannot when solid, only when molten or dissolved in water.

23
Q

Why can’t ionic compounds conduct electricity when solid?

A

The ions are fixed in position so there are no mobile charge carriers.

24
Q

Why can ionic compounds conduct electricity when molten or dissolved in water?

A

The solid ionic lattice breaks down.

The ions are now free to move as mobile charge carriers.

25
Q

Summarise properties of most ionic compounds.

A

High melting points and boiling points.
Tend to dissolve in polar solvents like water.
Conduct electricity only when molten or in aqueous solution.

26
Q

What is covalent bonding?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms.

27
Q

What actually is a covalent bond in terms of atomic orbital?

A

The overlap of atomic orbitals, each containing one electron, to give a shared pair of electrons.

28
Q

How does covalent bonding differ to ionic bonding?

A

In covalent bonding the attraction is localised. Attraction acts only on the shared pair of electrons and the nuclei of bonded atoms.

In ionic bonding the ion attracts in all directions in 3 dimensions.

29
Q

How can covalent bonding be displayed?

A

Dot and cross diagram

30
Q

What is a double bond?

A

The electrostatic attraction is between 2 shared pairs of electrons, and the nuclei of the bonding atoms

31
Q

What is a triple bond?

A

The electrostatic attraction is between 3 shared pairs of electrons and the nuclei of the bonding atoms.

32
Q

What is a dative covalent bond?

A

When both electrons in the shared pair are donated by one of the bonding atoms.

33
Q

Give an example of a dative covalent bond.

A

Ammonia donates its lone pair of electrons to H+ to form an ammonium ion, NH4+

34
Q

What is average bond enthalpy?

A

Measurement of the strength of a covalent bond.

Chemistry (20 decks)

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