Chapter 3:Metals

Question 1

metallurgy

Answer 1

science of modifying metals.

Question 2

5 careers/categories metals are required.

Answer 2

• construction
• agriculture
• art
• medicine
• transport

Question 3

3 Metal ages in order

Answer 3

• Copper Age (5000-3000BCE)
• Bronze Age (3000-1000BCE)
• Iron Age (from 1000 BCE)

Question 4

4 Properties of metals

Answer 4

1) have a range of melting points and relatively high boiling points
2) are good conductors of electricity
3) are good conductors of heat
4) generally have high densities

Question 5

2 Exception of the properties of metals

Answer 5

1) Mercury = liquid in room temp, unusually low melting point

2) Alkali Metals (group 1) = different from other metals
- soft enough to be cut by knife
- react vigorously with water to produce hydrogen gas.

Question 6

5 Common metallic CHARACTERISTICS

Answer 6

1) malleable- can be shaped by beating or rolling
2) ductile - can be drawn into a wire
3) lustrous or reflective - when freshly cut or polished
4) are often hard with high tensile strength
5) have low ionisation energies and electronegativities

Question 7

octet rule

Answer 7

electrons combine so there are 8 electrons in the outer shells.

Question 8

are metals or non metal atoms larger in ions?

is the core charge higher in metals or non metals?

Answer 8

metal atoms = larger than non metallic atom
core charge= lower in metals

ionisation energies is lower in metals than for non metals in the same period

Question 9

what are cations?

Answer 9

• POSITIVE IONS

- lose electrons in valence shells

Question 10

how to determine the charge

Answer 10

1) determine the number of protons and electrons in atom
2) figure out the shell configuration
3) amount of electrons - number of valence electrons
4) Cation charge = number of protons - number of electrons (without the valence electons)

Question 11

5 points about Transition metals

Answer 11

• between group 2-13
• known as d-block
• have unfilled d-subshells
• are usually silver coloured and similar in appearance
• transition metal compounds tend to be brightly coloured

Question 12

4 Properties of transition metals

Answer 12

1) they tend to be harder
2) they have higher densities
3) they have higher melting points
4) some have strong magnetic properties

Question 13

why are transition metals hard , have higher densities and higher melting points?

Answer 13

• atoms of transition metals are smaller in size due to their greater core charge
• this allows them to pack together tightly with stronger bonds.

Question 14

metals are usually hard and then to have high melting points. What does this tell us about it’s structure.

Answer 14

the forces between the particles must be strong

Question 15

Metals conduct electricity in the solid and molten liquid state. What does this tell us about it’s structure?

Answer 15

metals have charged particles that are free to move

Question 16

Metals are malleable and ductile

What does this tell us about it’s structure.

Answer 16

the attractive forces between the particles must be stronger than the repulsive forces between the particles when the layers of particles are moved

Question 17

metals generally have high densities

What does this tell us about it’s structure.

Answer 17

the particles are closely packed in a metal

Question 18

metals are good conductors of heat

What does this tell us about it’s structure.

Answer 18

there must be a way of quickly transferring energy through a metal object

Question 19

Metals are lustrous or reflective

What does this tell us about it’s structure.

Answer 19

free electrons are present, so metals can reflect light and appear shiny

Question 20

metals tend to react by losing electrons

What does this tell us about it’s structure.

Answer 20

electrons must be relatively easily removed from metal atoms

Question 21

3 things metal bonding model must include

Answer 21

1) charged particles that are free to move and conduct electricity
2) strong forces of attraction between atoms throughout the metal structure
3) some electrons that are relatively easily removed.

Question 22

lattice

Answer 22

tightly packed arrangement

Question 23

delocalised

Answer 23

spread throughout a large area.

- in the metallic bonding model positive metal cations are surrounded by a sea of delocalised electrons

Question 24

metals are hard and have relatively high boiling points

explanation?

Answer 24

strong electrostatic forces of attraction between positive metal ions and the sea of delocalised electrons holds the metallic lattice together

Question 25

metals are good conductors of electricity.

Explanation>

Answer 25

free moving delocalised electrons will move towards a positive electrode and away from a negative electrode in an electric circuit.

Question 26

metals are malleable and ductile

Answer 26

when a force causes metal ions to move past each other, layers of ions are still held together by the delocalised electrons between them

Question 27

what is the metallic bonding model?

Answer 27

is the electrostatic force of attraction between a lattice of positive ions and delocalised valence electrons. The lattice of cations is surrounded by a sea of delocalised electrons

Question 28

3 limitations of metallic bonding

Answer 28

• range of melting points, hardness and densities of different metals
• differences in electrical conductivities of metals
• magnetic nature of metals such as cobalt, iron and nickel.

Question 29

which elements are more reactive in water?

Answer 29

• metals in group 1 are more reactive in water compared to group 2
• going down a group the reactivity increases
• going across a period the reactivity decreases.

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