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National 5 Chemistry > Bonding > Flashcards

Bonding Flashcards

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
When do non metals conduct electricity
they don't ( except graphite)
26
When do ionic compounds conduct electricity
in aqueous form but not when in solid form
27
Why do ionic substances only conduct in solution
the charged particles are free to move and carry the electricity
28
Are ionic compounds solid at room tmperature
yes
29
What state are covalent compounds at room temperature
solids, liquids or gasses
30
How strong are metallic bonds
very
31
What happens when a solid metal melts
the atoms move and become more disarranged
32
How can atoms move in the strong metallic bonds
Break the bonds
33
What are ions in a crystal lattice held together with
strong forces of attraction
34
When an ionic solid melts the ions move apart. The amount of energy needed to separate the ions is ____
High
35
Can covalent bonds break
not easily although their inter molecular forces are weak and easily broken
36
What are the 2 types of compounds
Molecular (covalent) and ionic
37
Why can covalent molecular and network substances not conduct electricity
they do not have charged particles that are free to move and carry electricity
38
What happens when ionic compounds dissolve in water
the ions separate and are surrounded by water molecules
39
Name the 7 diatomic elements
Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine Iodine
40
Why are covalent bonds strong
the force of attraction between the positive nuclei and the negative electrons in the overlap region is strong
41
Do ionic compounds have high or low melting points
high since at melting point, strong ionic bonds within the lattice need to be broken in order to overcome the lattice
42
Do covalent substances have high or low melting points
low because the attractions between molecules (inter molecular forces)are easy to overcome when the substance changes state
43
Do covalent network compounds have high or low melting points
Millions of strong covalent bonds need to be broken for a change of state so high
44
Do covalent molecular compounds have high or low melting points
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
What does the term diatomic molecule mean
Diatomic- 2 atoms joined together molecule- atoms joined together by a covalent bond
46
name the 2 types of covalent structures
network molecular
47
describe the bonds in covalent substances
Bonds inside the molecules are strong Bonds between molecules are weak forces of attraction
48
Explain why discrete covalent substances have low melting and boiling points
Weak bonds in between molecules are broken where there is a change of state, no strong covalent bonds
49
Describe the structure of covalent network substances
Complex structure of millions of strong covalent bonds
50
Why can graphite conduct electricity
it has free moving electrons
51
What does the ending -ide tell u about a compound and give an exception
Contains 2 elements only except hydroxide which is a group ion
52
What does the name ending -ite or -ate tell u about a compound
2 elements present and oxygen
53
Some covalent substances are made up of ____________________ . These different molecules are held together by weak forces known as ______________________
discrete molecules inter-molecular forces
54
What is the definition for the word DIATOMIC
exist as 2 atoms covalent bonded

National 5 Chemistry (13 decks)

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