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Geography climate > Chemistry > Flashcards

Chemistry Flashcards

YR10

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1
Q

Most stable atoms

A

Noble gases

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2
Q

Ionic Bond

A

String electro static forces of attraction between oppositely charged ions

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3
Q

What to atoms do to become more stable?

A

Lose or gain electrons

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4
Q

Group and how many they will lose

A

Group 1 -LOSE 1
G2-LOSE 2
G3-LOSE 3
G5-GAIN 3
G6-GAIN 2
G7-GAIN 1

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5
Q

Positively charged ion

A

Cations

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6
Q

negatively charged ions

A

anions

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7
Q

Charge if loses or gains

A

LOSE 1= 1+
LOSE 2= 2+
LOSE 3= 3+
GAIN 3= 3-
GAIN 2= 2-
GAIN 1= 1-

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8
Q

How are ionic bonds formed

A

when two elements transfer electrons

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9
Q

Ion

A

atom or group of atoms with electrical charge
charged particle

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10
Q

Giant ionic lattice

A

Billions + Billions of ions in a regular arrangement(rows and columns)
forms crystals

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11
Q

ionic compound contains..

A

ions

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12
Q

Why is a lot of energy needed to break ionic bonds

A

the electrostatic force of attractions of charged ions are strong needing a lot of energy to break/overcome

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13
Q

Why do ionic compound have have high mp + bp ?

A

have strong bonds needing lots of energy =why they must be heated temps so the giant ionic lattice is broken

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14
Q

Why do some ions need more energy than others

A

Have more than one charge needing more energy

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15
Q

Do ionic compound conduct electricity?

A

when they are molten or dissolved in water
DON’T CONDUCT ELECTRICITY IN SOLID STATE

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16
Q

Why can they only conduct in molten state

A

Able to move freely unlike in solids where they can only vibrate
so they cat carry electrical charge

17
Q

Covalent bonds

A

Between non metals and non metals

18
Q

Ionic bonding

A

Metals + non-metals

19
Q

What happens in Covalent bonding

A

Cant transfer electrons in non-metals so they share

20
Q

How is covalent bonding formed

A

Between non-metals
electrons shared between two atoms
covalent bonds between molecules are strong
strong electrostatic forces of attraction between positive nucleus and negative electrons

21
Q

Bonds

A

1 electron between 2 atoms-single bond
2 pairs of electrons-double
3 pairs of electrons-triple

22
Q

Molecular compounds

A

some compounds exist as molecules-distinct groups of atoms joined together
covalent, simple molecular structures
e.g H2O

23
Q

MP + BP of molecular compounds

A

Covalent bonds are strong forces of attraction
HOWEVER
also have weak forces of attraction between molecules(INTERMOLECULAR FORCES)

LOW MP + MP

24
Q

Do molecular compoun?ds conduct electricity

A

Simple molecules have no overall charge (no mobile charge) + cant carry electrical current
electrons cant flow

25
Q

Monomers

A

small SIMPLE molecules that can be joined in a chain to form a polymer

26
Q

polyethene

A

ethene monomer molecules(gas a room temp)join to form polyethene,solid at room temp (stronger attractions)

27
Q

Polymers

A

Long polymers have more weak intermolecular forces
longer chains get tangled up so they have high MP + BP

28
Q

Allotropes

A

same type of atom but different structures

29
Q

4 allotropes of carbon

A

fullerens
graphene
diamond
graphite

30
Q

Fullerenes

A

simple molecules
each carbon covalently bonded to 3 other carbons
E.G buckministerfullerene that has 60 carbon atoms forming C60
weak intermolecular forces
makes them soft + slippery
delocalised electrons cant move freely bcz its molecular

31
Q

Graphene

A

NOT simple molecule
no fixed formula
each atom covalently bonded to 3 other carbons
covalent bonds make extremely strong+ is light
carry charge bcz of delocalised electrons that can move freely transfering energy

32
Q

Diamond

A

Giant molecular structures
hard + high mp + bp
useful in cutting tools +jewellery
Doesn’t conduct electricity
insoluble in water
Every carbon bonded to 4 other carbons with stong covalent bonds

33
Q

Graphite

A

Carbon atoms in layers
slippery
component of many lubricants + pencil lead
insoluble in water
high mp + bp
good conductor of electricity
each carbon bonded to 3 carbons =free electron(delocalised)

34
Q

metallic structure

A

atoms same size + packed close together
forming giant lattice structure
outer shell electrons become delocalised leaving giant ionic lattice of + metals with ‘sea’of delocalised electrons.

35
Q

Metallic bonding

A

electrostatic attractions between + metal ions and - delocalised electrons

strong so have high mp + bp

36
Q

Why are metals malleable

A

The layers of ions slide over each other and delocalised electrons hold the positive ions together so metal changes shape instead of breaking

37
Q

conductivity in metals

A

Conductivity increases with the charge
higher the charge stonger the bond and electrical conductivity

38
Q

Hydroxide
Carbonate
Sulfate
Nitrate
Ammonium
Phosphate

A

OH-
CO32-
SO42-
NO3-
NH4+
PO43-

39
Q

Ionic
covalent
metallic

A

metal +non-metal>giant
non-metal+non-metal>giant/simple
metal atoms>giant

Geography climate (4 decks)

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