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National 5 Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

How many MAIN types of bonding are seen in elements and compounds

A

3

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2
Q

What are the elements like in COVALENT bonds

A

non-metals

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3
Q

What are the elements like in IONIC bonds

A

metals + non-metals

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4
Q

What are the elements like in METALLIC bonds

A

metals

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5
Q

what is a covalent bond

A

an attraction between 2 atoms where a shared pair of electrons form a bond

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6
Q

What holds the negatively charged electrons in a covalent bond

A

the positive nuclei

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7
Q

What is a molecule

A

a substance when 2 or more atoms are held together by covalent bond

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8
Q

How many elements exist as molecules (they are also known as the diatomic elements)

A

7

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9
Q

How many shared pairs of electrons form a SINGLE covalent bond

A

1

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10
Q

How many shared pairs of electrons form a DOUBLE covalent bond

A

2

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11
Q

How many shared pairs of electrons form a TRIPLE covalent bond

A

3

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12
Q

What are covalent network structures

A

compounds made up of non metal atoms which are joined together by covalent bonds in a giant network structure

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13
Q

Give 3 examples of Covalent network structures

A

Carbon- Diamond and graphite
Silicon Dioxide (sand)

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14
Q

Can covalent network structures dissolve in water?

A

no but they can dissolve in other covalent liquids

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15
Q

Do ions have a charge

A

yes

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16
Q

Do metal atoms gain or lose electrons

A

Metal atoms always LOSE electrons to form POSITIVE metal ions

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17
Q

Do non-metal atoms gain or lose electrons

A

Non-metal atoms always GAIN electrons to form NEGATIVE metal ions

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18
Q

How are ionic compounds normally formed

A

when metal and non-metal elements combine

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19
Q

What is ionic bonding, by defenition

A

the electrostatic attraction between ions of opposite charge

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20
Q

What do ionic compounds exist as?

A

a giant lattice structure of oppositely charged ions

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21
Q

How do metallic structures exist as?

A

a giant metallic lattice of positively charged ions and delocalised outer electrons

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22
Q

What is electricity

A

the flow of charged particles ( electrons or ions)

23
Q

What needs to happen to substances for them to conduct

A

must have charged particles which are free to move and carry the electricity

24
Q

When do metals conduct electricity

A

when in liquid or solid

25
Q

When do non metals conduct electricity

A

they don’t ( except graphite)

26
Q

When do ionic compounds conduct electricity

A

in aqueous form but not when in solid form

27
Q

Why do ionic substances only conduct in solution

A

the charged particles are free to move and carry the electricity

28
Q

Are ionic compounds solid at room tmperature

A

yes

29
Q

What state are covalent compounds at room temperature

A

solids, liquids or gasses

30
Q

How strong are metallic bonds

A

very

31
Q

What happens when a solid metal melts

A

the atoms move and become more disarranged

32
Q

How can atoms move in the strong metallic bonds

A

Break the bonds

33
Q

What are ions in a crystal lattice held together with

A

strong forces of attraction

34
Q

When an ionic solid melts the ions move apart. The amount of energy needed to separate the ions is ____

A

High

35
Q

Can covalent bonds break

A

not easily although their inter molecular forces are weak and easily broken

36
Q

What are the 2 types of compounds

A

Molecular (covalent) and ionic

37
Q

Why can covalent molecular and network substances not conduct electricity

A

they do not have charged particles that are free to move and carry electricity

38
Q

What happens when ionic compounds dissolve in water

A

the ions separate and are surrounded by water molecules

39
Q

Name the 7 diatomic elements

A

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine

40
Q

Why are covalent bonds strong

A

the force of attraction between the positive nuclei and the negative electrons in the overlap region is strong

41
Q

Do ionic compounds have high or low melting points

A

high since at melting point, strong ionic bonds within the lattice need to be broken in order to overcome the lattice

42
Q

Do covalent substances have high or low melting points

A

low because the attractions between molecules (inter molecular forces)are easy to overcome when the substance changes state

43
Q

Do covalent network compounds have high or low melting points

A

Millions of strong covalent bonds need to be broken for a change of state so high

44
Q

Do covalent molecular compounds have high or low melting points

A

low since at melting point, no covalent bonds are broken since they are strong. although heir inter molecular forces are weak and easily broken

45
Q

What does the term diatomic molecule mean

A

Diatomic- 2 atoms joined together
molecule- atoms joined together by a covalent bond

46
Q

name the 2 types of covalent structures

A

network
molecular

47
Q

describe the bonds in covalent substances

A

Bonds inside the molecules are strong
Bonds between molecules are weak forces of attraction

48
Q

Explain why discrete covalent substances have low melting and boiling points

A

Weak bonds in between molecules are broken where there is a change of state, no strong covalent bonds

49
Q

Describe the structure of covalent network substances

A

Complex structure of millions of strong covalent bonds

50
Q

Why can graphite conduct electricity

A

it has free moving electrons

51
Q

What does the ending -ide tell u about a compound and give an exception

A

Contains 2 elements only except hydroxide which is a group ion

52
Q

What does the name ending -ite or -ate tell u about a compound

A

2 elements present and oxygen

53
Q

Some covalent substances are made up of ____________________ . These different molecules are held together by weak forces known as ______________________

A

discrete molecules
inter-molecular forces

54
Q

What is the definition for the word DIATOMIC

A

exist as 2 atoms covalent bonded

National 5 Chemistry (13 decks)

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