Bonding

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

Card preview (24)

Front (Question)

The melting point of XeF4 is higher than the melting point of PF3 Explain why the melting points of these two compounds are different. In your answer you should give the shape of each molecule, explain why each molecule has that shape and how the shape influences the forces that affect the melting point.

Back (Answer)

• XeF4 4BP and 2LP around Xe • PF3 3BP and 1LP around P • XeF4 square planar • PF3 pyramidal • XeF4 has vdw forces and PF3 has dipole- dipole forces (and vdw) • Stronger/more intermolecular forces in XeF4 • Due to larger Mr

Front (Question)

Ionic bonding structure and bonding

Back (Answer)

strucutre = giant lattice bonding = strong ionic

Front (Question)

ionic bonding definition

Back (Answer)

• strong electrostatic forces of attraction • between oppositely charged ions

Front (Question)

physical properties of ionic compounds

Back (Answer)

• high MP/BP • electrical conductivity when aqueous • brittle

Front (Question)

covalent bonding structure and bonding

Back (Answer)

structure = simple covalent/macromolecular bonding = strong covalent

Front (Question)

covalent bonding definition

Back (Answer)

• shared pair of electrons • between two atoms

Front (Question)

properties of diamond

Back (Answer)

• tetrahedral • each C atom forms 4 covalent bonds • high MP • hard • non-conductor of electricity (no delocalised electrons)

Front (Question)

properties of graphite

Back (Answer)

• each carbon forms 3 covalent bonds • each carbon has one free delocalised electron • layers held by weak VDW • soft (layers can slide over each other) • high MP (strong covalent bonds) • conducts electricity due to delocalised electrons

Front (Question)

define co-ordinate bonding

Back (Answer)

• shared electron pair • from same atom

#10

Front (Question)

metallic bonding structure and bonding

Back (Answer)

structure = giant lattice bonding = strong metallic bonds

#11

Front (Question)

why does Mg have stronger bonding than Na

Back (Answer)

• Mg2+ ions smaller than Na+ ions • Mg2+ greater charge • more delocalised electrons • attraction between Mg2+ and delocalised electrons stronger

#12

Front (Question)

properties of metals

Back (Answer)

• electrical and thermal conductors (delocalised electrons) • strong (strong forces of attraction) • malleable and ductile • high MP/BP

#13

Front (Question)

calcium carbonate formula

Back (Answer)

CaCO3

#14

Front (Question)

Magnesium nitrate formula

Back (Answer)

Mg(NO3)2

#15

Front (Question)

Zinc phosphate formula

Back (Answer)

Zn3(PO4)2

#16

Front (Question)

Sodium sulphide formula

Back (Answer)

Na2S

#17

Front (Question)

Copper (I) hydroxide formula

Back (Answer)

CuOH

#18

Front (Question)

Aluminium dichromate formula

Back (Answer)

Al2(Cr2O7)3

#19

Front (Question)

Lead (II) sulphate formula

Back (Answer)

PbSO4

#20

Front (Question)

Silver (I) iodide formula

Back (Answer)

AgI

#21

Front (Question)

Ammonium carbonate formula

Back (Answer)

(NH4)2 CO3

#22

Front (Question)

Potassium oxide formula

Back (Answer)

K2O

#23

Front (Question)

state structure for iodine and graphite

Back (Answer)

iodine = simple molecular graphite = giant covalent/macromolecular

#24

Front (Question)

explain why graphite has high MP

Back (Answer)

lots of strong covalent bonds need to be broken