Structure and Bonding - Facts

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

Card preview (24)

Front (Question)

State which force oppositely charged particles experience

Back (Answer)

Electrostatic force

Front (Question)

State the elements involved in metallic bonding

Back (Answer)

Metals

Front (Question)

Describe the bonding in metallic bonding

Back (Answer)

Positive metal ions electrostatically attracted to sea of delocalised electrons.

Front (Question)

Describe the structure in metallic bonding

Back (Answer)

A regular arrangement of metal cations surrounded by a sea of delocalized electrons

Front (Question)

Explain why metals can conduct electricity

Back (Answer)

Have delocalised electrons which can move through the structure and carry charge

Front (Question)

Explain why metals have high melting points

Back (Answer)

• Strong electrostatic attraction • That acts in all directions • Between many oppositely charged ions • Which requires lots of energy to overcome

Front (Question)

Explain why metals are malleable

Back (Answer)

Layers of atoms can easily slide over each other

Front (Question)

Explain the trend in conductivity

Back (Answer)

Across a period, more electrons, which can move through the structure carrying charge

Front (Question)

Explain the trend in melting point in metals along a period

Back (Answer)

Across a period, more electrons, so more electrostatic attraction and more energy to melt

#10

Front (Question)

Explain why alloys are stronger than pure metals

Back (Answer)

Alloys have different sized atoms that disrupt the regular arrangement, making it harder for layers to slide

#11

Front (Question)

State the elements involved in ionic bonding

Back (Answer)

Metals and non-metals

#12

Front (Question)

Describe the bonding in ionic bonding

Back (Answer)

Oppositley charged ions which are electrostatically attracted

#13

Front (Question)

Describe the structure in ionic bonding

Back (Answer)

Giant, ionic lattice

#14

Front (Question)

Explain how ionic compounds can conduct electricity

Back (Answer)

When dissolved in water or molten, ions are free to move and carry charge

#15

Front (Question)

Explain why ionic compounds have high melting points

Back (Answer)

Strong electrostatic forces between many oppositely charged ions require a lot of energy to break

#16

Front (Question)

Describe how an ionic bond forms

Back (Answer)

• Metals transfer electrons -become positive ion • To non-metals- become negative ion • Strong electrostatic attraction between negatively charged ions

#17

Front (Question)

State the elements involved in covalent bonding

Back (Answer)

Non-metals

#18

Front (Question)

Describe the bonding in covalent bonding

Back (Answer)

Sharing of pairs of electrons between non-metal atoms

#19

Front (Question)

Describe the structure of giant covalent structures

Back (Answer)

Giant covalent lattice

#20

Front (Question)

Give the typical properties of simple covalent structures

Back (Answer)

• Simple: low melting and boiling points, poor conductivity

#21

Front (Question)

Describe the structure of simple covalent structures

Back (Answer)

Simple, (small), discrete molecules

#22

Front (Question)

Give the typical properties of giant covalent structures

Back (Answer)

high melting and boiling points, generally poor conductivity

#23

Front (Question)

Give 2 examples of giant covalent structures

Back (Answer)

• Diamond • Sand

#24

Front (Question)

State which force is responsible for the boiling point of simple covalent structures

Back (Answer)

Intermolecular forces