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3.1.3 Bonding

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

#1
Front (Question)

Ionic Bonding [definition]:

Back (Answer)

The electrostatic attraction between oppositely charged ions in a lattice

#2
Front (Question)

Covalent Bonding [definition]:

Back (Answer)

A shared pair of e⁻s with opposite spins - one e⁻ donated by each atom

#3
Front (Question)

Sulphate formula:

Back (Answer)

SO₄²-

#4
Front (Question)

Hydroxide formula:

Back (Answer)

OH−

#5
Front (Question)

Nitrate formula:

Back (Answer)

NO₃⁻

#6
Front (Question)

Giant Ionic lattice [2]:

Back (Answer)

• Sodium Chloride - Magnesium oxide

#7
Front (Question)

Covalent simple molecular structures [5]:

Back (Answer)

• Iodine • Ice • Carbon dioxide • Water • Methane

#8
Front (Question)

Giant Covalent structures [4]:

Back (Answer)

• Diamond • Graphite • Silicon dioxide • Silicon

#9
Front (Question)

Ionic boiling and melting points [2]:

Back (Answer)

• high- because of giant lattice of ions with strong electrostatic forces between oppositely charged ions • requires lot of energy to break

#10
Front (Question)

Ionic Solubility in water:

Back (Answer)

Generally good

#11
Front (Question)

Ionic compound conductivity (when solid): [2]

Back (Answer)

• poor - ions can’t move/ fixed in lattice

#12
Front (Question)

Ionic compound conductivity (when molten): [2]

Back (Answer)

• Good - Ions can move freely

#13
Front (Question)

Co-ordinate/ Dative Covalent bond [definition]:

Back (Answer)

A bond that contains a shared pair of electrons with both electrons supplied by one atom.

#14
Front (Question)

Simple Covalent compound boiling and melting points:

Back (Answer)

low- because of weak intermolecular forces between molecules (specify type e.g van der waals/hydrogen bond)

#15
Front (Question)

Simple covalent compound solubility in water:

Back (Answer)

Generally poor

#16
Front (Question)

Simple covalent compound conductivity (when solid): [2]

Back (Answer)

• poor • no ions to conduct and electrons are localised (fixed in place)

#17
Front (Question)

Simple covalent compound conductivity (when molten): [2]:

Back (Answer)

• Poor - No ions

#18
Front (Question)

Giant Covalent compound boiling and melting points:

Back (Answer)

High- because of many strong covalent bonds in macromolecular structure (requires a lot of energy to break many strong bonds)

#19
Front (Question)

Giant covalent compound solubility in water:

Back (Answer)

Insoluble

#20
Front (Question)

Giant covalent compound conductivity (when solid): [2]:

Back (Answer)

• diamond and sand = poor because electrons are localised and can’t move • graphite = good, has free delocalised electrons between layers to conduct

#21
Front (Question)

Giant covalent compound conductivity (when molten):

Back (Answer)

Poor

#22
Front (Question)

Metallic bonding boiling and melting points:

Back (Answer)

high- strong electrostatic forces between positive ions and sea of delocalised electrons

#23
Front (Question)

Metallic bonding solubility in water:

Back (Answer)

Insoluble

#24
Front (Question)

Metallic bonding conductivity (when solid): [2]:

Back (Answer)

• good - delocalised electrons can move through structure