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Chemisty > S3 EXAM > Flashcards

S3 EXAM Flashcards

1
Q

Mono

A

One

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2
Q

Di

A

Two

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3
Q

Tri

A

Three

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4
Q

Tetra

A

Four

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5
Q

What substances form together to make ionic bonds

A

Metal and non-metals

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6
Q

Ionic bonding

A

It is an electrostatic force of attraction between oppositely charged ions

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7
Q

Strength of ionic compound

A

Strong

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8
Q

Why do atoms gain or lose electrons

A

They are more stable with a full outer shell of electrons

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9
Q

What happens when metal atoms form ions

A

They lose an electron to form positive ions

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10
Q

How do you work out how many electrons a metal loses when when it forms an ion

Why do metal ions do this

A

A metal loses electrons equal to the number of electrons in the outer shell

They are more stable with a full outer shell of electrons

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11
Q

What happens to non-metal atoms when they form ions

A

They always gain electrons to become megitive ions

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12
Q

What substances have metallic bonding

A

Metals

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13
Q

Metallic bonding

A

Electrostatic attraction between positively charged atom cores or ions and delocalised electrons

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14
Q

Strength of metallic bonds

A

Strong

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15
Q

What elements form covalent bonds

A

Non-metal atoms

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16
Q

Covalent bonds

A

Shared pair of electrons

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17
Q

What holds the atoms together in covalent bonds

A

The shared pair of electrons is attracted to both positive nuclei

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18
Q

What is a molecule

A

A group of atoms held together by covalent bonds

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19
Q

What is a diatomic molecule

A

A molecule that contains two atoms

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20
Q

What is meant by a discreet molecular substance

A

One that exists with separate molecules

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21
Q

Strength of covalent bonds

A

The covalent bonds inside molecules are strong whereas the forces of attraction are week

22
Q

Covalent network

A

A giant structure where atoms are covalently bonded together e.g silicon, carbon, graphite

23
Q

Electric current

A

A floe of charged particles

24
Q

What charged particles can carry a current

A

Freely moving/delocalised electrons or ions

25
Q

Why do covalent compounds not conduct electricty

A

Covalent compounds consist of molecules that are unchanged, they contain no charged particles to carry an electric current

26
Q

In what state will ionic compounds conduct

A

Ionic compounds don’t conduct in solid state but when molten or dissolved in water

27
Q

Why do metals have high melting and boiling points

A

Strong metallic bonds are broken as metals melt and boil. These bonds are strong as the delocalised electrons are attracted to many surrounding positive ion cores

28
Q

Why do ionic compounds have a high melting and boiling point

A

Strong ionic bonds must be broken as ionic compounds melt and boil. The ionic bonds are strong as there is a strong electrostatic force of attraction between positive and negative ions

29
Q

Why do covalent network structures have high melting and boiling point

A

Only the weak forces of attraction between molecules are broken when these substances melt/biol. the strong covalent bonds in the molecule are NOT broken

30
Q

How soluable are ionic substances in water

A

They are usually souable

31
Q

What is a vertical columb of element called in the periodic table

A

A group

32
Q

What is a horizontal group of elements called

A

A period

33
Q

In what ways are elements that are in the same group similiar

A

Similar chemical properties

Same number of electrons on outer shell

34
Q

Alkali metals

A

Very reactive metals

35
Q

Halogens

A

Very reactive non-metals

36
Q

Noble gasses

A

Very unreactive non-metals

37
Q

Why are atoms neutral

A

They contain the same amount of positive protons and negative electrons

38
Q

What is used to put the elements in order in the periodic table

A

In order of atomic mass

39
Q

What is the atomic number

A

The number protons in the nucleus

40
Q

What is the mass number

A

The number proton plus neutrons in the nucleus

41
Q

How to calculate the number of netrons

A

Mass number - atomic mass

42
Q

What is an isotope

A

Atoms of the element with different mass numbers but same atomic number

43
Q

Relative atomic mass

A

The average mass of an element taking into propotion/ abundance of each isotope present

44
Q

4 factors that can effect the rate of a chemical reaction

A

Concentration
Temperature
Particle size
Catalyst

45
Q

Collision theory

A

In order for a reaction to take place reactant particles must collide with each other

46
Q

Catalyst

A

A catalyst is a substance that can be added to a chemical reaction to increase the rate. Without getting used up

47
Q

4 ways to measure the rate of chemical reactions

A

Measure volume of gas collected
Measure mass loss
Measure pH change
Measure colour change

48
Q

Why do acids conduct electricity

A

Acids produce the hydrogen ion when dissolved in water. These ions when in water act as charge carriers and conduct

49
Q

What type of bonding do acids have

A

Ionic bonding

50
Q

Why do alkalis conduct electricity

A

They contains hydroxide ion. Theses ions conduct electricity

Chemisty (18 decks)

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