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C2 - Chemistry > Structure And Bonding > Flashcards

Structure And Bonding Flashcards

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1
Q

What is the charge on an electron

A

-

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2
Q

What is the change on a neutron

A

0 charge

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3
Q

What is the mass of: protons neutrons and electrons?

A

Protons - 1
Neutrons - 1
Electrons - 1/2000 (approx)

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4
Q

How are elements ordered in the periodic table?

A

They are arranged in atomic number

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5
Q

What is atomic number?

A

Number of protons

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6
Q

What is atomic mass

A

Number of protons and neutrons

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7
Q

Is the atomic number or atomic mass on top on the periodic table?

A

The atomic mass is on top

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8
Q

Why are atoms electrically neutral?

A

Because they have the same number of positive and negative charges ( protons and electrons)

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9
Q

What is the attraction of positive and negative ions?

A

The electrostatic force of attraction

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10
Q

What is the charge on a proton?

A

Positive

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11
Q

What is the relationship between the number of electrons in the highest energy level and the group number?

A

The number of electrons in the outer shell belong to the same group on the periodic table

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12
Q

Why do atoms react and bond?

A

In order to gain a full outer shell to become stable

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13
Q

How are the ions held together in eg solid magnesium oxide?

A

They are held together by the electrostatic force of attraction between positive and negative ions

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14
Q

Property of diamond?

A

Hardness

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15
Q

What is an element?

A

A substance which contains one type of atom

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16
Q

What is the difference between a mixture and a compound?2

A

Mixtures contain more than one element

Compounds are chemically bonded mixtures aren’t

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17
Q

Why are metals malleable and ductile?

A

Because metals are arranged in layers

So the layers of ions can slide over each other

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18
Q

Why do metals conduct electricity?

A

Because they are held together in an see of delocalised electrons but the electrons are able to move because the electrons are free to carry charge

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19
Q

Why do metals have high melting/boiling points?

A
  • strong electrostatic is between positive ions and electrons that take a lot of energy to break
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20
Q

What is the arrangement of metal atoms?

A

Closely packed in layers

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21
Q

Physical properties of metals?6

A
  • good conductor of heat and charge
  • shiny
  • generally hard (and solid)
  • malleable
  • alloys
  • generally grey
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22
Q

Two elements with giant covalent structures?

A

Diamond and carbon

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23
Q

What state are ionic substances at at room temperature?

A

Solid

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24
Q

Why do ionic substances have high boiling points?3

A

Because they form strong bonds
Because of the electrostatic force of attraction oppositely charged ions
so a lot of energy is required to break them

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25
Q

Do ionic substances have low melting points?

A

No they are high

26
Q

Why will ionic compounds conduct electricity when molten or in solution?

A

Because their ions can move freely and thus carry charge through the liquid

27
Q

At room temperature what are simple molecules?

A

They are liquids or gases

28
Q

Why don’t simple molecules conduct electricity? 3

A

There is overall charge on a simple molecule
so they can’t carry electrical charge

& no free electrons

29
Q

Why do substances made up of simple molecules have low boiling points?3

A
  • between molecules
  • there are weak intermolecular forces
  • not much energy is required to break them and boil the substance
30
Q

Describe an ionic lattice? 3

A
  • regular arrangement ( in rows)
  • held together by an electrostatic force of attraction
  • between oppositively charged ions
31
Q

In a simple molecule what is strong and what is weak?2

A

The covalent bonds are strong

The forces between molecules are weak

32
Q

Examples of simple molecules? 4

A

CO
HCl
CO2
H2

33
Q

Physical properties of diamond?4

A
  • very hard
  • very high boiling/melting point
  • insoluble in water
34
Q

Physical properties of graphite?3

A

Soft
Slippery
Conducts electricity

35
Q

Why is graphite slippery?3

A

There are weak intermolecular forces between the layers so
They can then slide over eachother
Making graphite soft and slippery

36
Q

Why is diamond hard?4

A

The atoms in diamond form a giant structure
They form strong covalent bonds
They form 4 bonds
So lots of energy is required to break the bonds

37
Q

Why can graphite conduct electricity?

A
  • it only makes three bonds to Carbon
  • this leaves a delocalised electron ( because it is arranged in layers)
  • can travel between the layers carrying charge
38
Q

Why can’t diamond conduct electricity? 2

A
  • Diamond does not have delocalised (free) electrons

- because they are all used in bonding

39
Q

How many bonds to carbon does diamond/graphite make?

A

4 and 3

40
Q

Examples of giant covalent structures?3

A

Silicon dioxide
Diamond
Graphite

41
Q

Describe the bonding in metals?

A

The bonding is strong because of the electrostatic force of attraction between ions and electrons

42
Q

What is a giant covalent structure?

A

A huge 3D network of covalently bonded atoms eg diamond or graphing

43
Q

What is a covalent bond?

A

A shared pair of electrons

44
Q

How is a covalent bond formed?3

A
  • When an atom wants to become stable
  • it can covalently bond to share electrons between the atoms
  • to form a full outer shell
45
Q

explain the bonding in giant covalent structures?4

A
  • Lots of bonds
  • very strong bonds
  • covalent bonds
  • held together in regular giant lattices
46
Q

Why is graphite softer than diamond?4

A
  • graphite has weak intermolecular forces
  • graphite is in layers that can slide over eachother
  • in diamond each atom had no free electrons as in bonded to 4
  • so no carbon atoms can slide over eachother
47
Q

What are nano particles?

A

Particles of size 1-100 nm

48
Q

Why does carbon dioxide have a low boiling point?3

A
  • carbon dioxide is a simple molecule
  • there are weak intermolecular forces between the molecules
  • so not much energy is needed to break them
49
Q

How does a positively charged hydrogen ion change into a hydrogen atom?

A

Gains one electron

50
Q

Why is silicon dioxide a suitable material for lining furnaces?

A
  • high melting point
  • lot of energy needed to break its bonds
  • because it has strong bonds
  • because it is a giant structure
51
Q

Describe the structure of a metal?

A

Sea of delocalised electrons

Positively charged metal ions

52
Q

Describe the structure and bonding of a metal?

A

Positive ions
Sea of delocalised electrons
That carry charge
Giant lattice

53
Q

Why use a certain metal for dental braces?

A

Shape memory alloy

54
Q

How does an ion form?

A

When atoms form chemical bonds by transferring electrons

55
Q

Alkali metals react with non metals to form what?

A

Ionic compounds

In which the metal ions has a single positive charge

56
Q

What does a compound contain?

A

Two or more elements which are chemically combined

57
Q

What is a compound?

A

Substances in which 2 or more elements are chemical combined

58
Q

Why do ionic compounds have high melting and boiling points?

A

Because lots of energy is required to break the many strong bonds

59
Q

What do metals consist of?

A

Giant structure of atoms in a regular patterns

Delocalised electrons held in place by positive ions (electrostatic force of attraction)

60
Q

Describe force in ionic lattices?

A

The force exerted by an ion on other ions in the lattice acts equally in all directions

61
Q

Why are ionic structures held together so strongly?

A

Force exerted by an ion on other ions acts equally in all directions

C2 - Chemistry (5 decks)

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