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GCSE - chemistry > CC5,6,7- bonding > Flashcards

CC5,6,7- bonding Flashcards

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1
Q

how can you tell which group (column) an element is in?

A

the number of electrons in the outer shell

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2
Q

how can you tell which period (row) an element is in?

A

the number of shells the element has

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3
Q

What are isotopes?

A

Atoms of the same element that have different numbers of neutrons

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4
Q

how do you calculate relative atomic mass?

A

(% of isotope 1 x mass of isotope 1) + (% of isotope 2 x mass of isotope 2) / 100

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5
Q

give an example of ionic bonding

A

sodium chloride, NaCl (salt)

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6
Q

what happens when sodium and chlorine bond?

A

The sodium has one electron on its outer shell, which is transferred to the chlorine atom. This gives both a full outer shell, and the sodium becomes positively charged, while the chlorine has a negative charge.

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7
Q

what is an ion?

A

a charged atom

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8
Q

How do ions become charged

A

by gaining or losing NEGATIVLEY CHARGED electrons

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9
Q

properties of ionic compounds (7)

A
  • giant lattice structure
  • attraction between + and - ions
  • conduct electricity when molten/ disolved in water
  • electrons can move
  • high melting and boiling point
  • electrostatic attraction
  • between a metal and non-metal
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10
Q

what is electrostatic attraction?

A

when oppositely charged ions are attracted to each other - non contact force.

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11
Q

What is covalent bonding?

A

bonding between non-metals, atoms gain a full outer shell of electrons by sharing pairs of electrons

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12
Q

properties of covalent compounds?

A
  • simple structure
  • low melting and boiling points due to weak intermolecular forces of attraction
  • never conducts electricity - electrons have no charge
  • between nonmetals
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13
Q

properties of metallic bonds

A
  • conduct electricity
  • strong giant structure
  • bonding between metals
  • high melting and boiling points
  • malleable - layers can move past eachother
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14
Q

how do metallic compounds conduct electricity if theyre solids?

A

the have delocalised electrons that can move within the structure

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15
Q

What is an allotrope?

A

Different forms of the same element

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16
Q

What are the allotropes of carbon?

A

diamond, graphite, graphene

17
Q

what are some physical properties of diamond?

A
  • hard
  • high melting point
  • insoluable in water
  • doesn’t conduct electricity
  • used in cutting tools
18
Q

what are some physical properties of graphite?

A
  • slippery (used a a lubricant)
  • brittle
  • insoluble in water
  • conducts electricity
19
Q

describe the structure of graphene?

A

giant covalent
type of fullerene
joined in hexagons
1 atom thick
conducts electricity well
4th electron can move

20
Q

describe the structure of graphite?

A

-layered
-every 4th electron is delocalised therefore can conduct electricity
-each carbon atom covalently bonded to 3 others
-weak imfoa, layers can slide past each other or be left behind when friction is applied

21
Q

describe the structure of diamond

A

giant covalent structure
strong bonds between all atoms
each carbon atom bonded to 4 others
very strong

22
Q

What are polymers?

A

Long chains of monomers joined together

23
Q

fullerenes (5)

A
  • molecules of carbon shaped in tubes or balls
  • made up of C atoms arranged in hexagons/ pentagons/ heptagons
  • simple structure
  • useful for transporting medicines around body
  • large SA good catalyst
24
Q

buckminsterfullerenes

A
  • molecular formula C60
  • hollow sphere of 20hex and 12pent
  • stable molecule
  • forms soft brown/black crystals
25
Q

nano-tubes

A
  • fullerenes
  • light
  • 1 atom thick
  • strong structure
  • conduct electricity
26
Q

what are nonotubes used in

A
  • strengthen materials w/o adding weight
  • robust, used in tennis rackets
27
Q

examples of some covalent compounds

A

water
carbon dioxide
methane

28
Q

what are giant covalent structures

A
  • all atoms bonded by strong covalent bonds
  • high mp and bp, lots of energy needed to break the bonds
  • don’t conduct electricity (no charged particles
29
Q

What is an ionic bond

A
  • The electrostatic forces of attraction between oppositely charged particles
  • The bond is formed when atoms lose or gain electrons in order to achieve a full outer shell

GCSE - chemistry (15 decks)

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