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Structure And Bonding Flashcards

(60 cards)

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1
Q

What are bonds?

A

Forces of attraction that hold atoms together

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2
Q

What do electrostatic forces hold together?

A

Oppositely charged ions forming an ionic bind between them

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3
Q

What is a lattice structure?

A

Billions of ions packed together in a regular repeating arrangement called a lattice structure

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4
Q

Why do ionic compounds have no overall charge?

A

They are electrically neutral

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5
Q

What is the ion formula of sodium?

A

Na+

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6
Q

What is the ion formula of lithium?

A

Li+

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7
Q

What is the ion formula for potassium?

A

K+

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8
Q

What is the ion formula for magnesium?

A

Mg2+

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9
Q

What is the ion formula for calcium?

A

Ca2+

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10
Q

What is the ion formula for aluminium?

A

Al3+

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11
Q

What is the ion formula for fluoride?

A

F-

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12
Q

What is the ion formula for chloride?

A

Cl-

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13
Q

What is the ion formula for bromide?

A

Br-

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14
Q

What is the ion formula for oxide?

A

O2-

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15
Q

What is the ion formula for sulfide?

A

S2-

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16
Q

What is the ion formula for phosphide?

A

P3-

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17
Q

What 2 conditions does a substance need to conduct electricity?

A
  • just contain charged particles

- these particles must be free to move

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18
Q

What are negative ions known as?

A

Anions

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19
Q

What are positive ions known as?

A

Cations

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20
Q

What are covalent bonds formed between?

A

Between non-metal atoms

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21
Q

How are covalent bonds produced?

A

By sharing pairs of electrons

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22
Q

What are electrostatic forces of attraction between?

A

Between the positive nuclei and negative electrons in bonded atoms

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23
Q

What is a compound?

A

A substance with atoms of more than one element

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24
Q

What do intermolecular forces hold together?

A

Water molecules

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25
What must be overcome when turning water into gas?
Intermolecular forces
26
What are monomers?
Small simple molecules that cane be joined in a chain to form a polymer
27
What do linger polymers have more of?
Intermolecular forces
28
Why do longer polymers have higher melting and boiling points than shorter ones?
The longer chains tend to get tangled up with one another
29
What are allotropes?
A different structural form of an element, e.g graphite and diamond are allotropes of carbon
30
What are molecules joined together by?
Covalent bonds
31
What is a fullerene?
A molecule in which each carbon atom is covalently bonded to three other carbon atoms, forming spheres or tube shapes
32
Do fullerenes have high or low melting points?
Low
33
Do fullerenes have strong or weak intermolecular forces?
Weak
34
Is graphene a good electrical conductor?
Yes
35
How thick is graphene
1 atom thick, making it the lightest known material
36
Why is graphene extremely strong?
Covalent bonds
37
Give 2 examples of covalent, giant molecular structures
Diamond and graphite
38
Why do graphite and diamond have high melting points?
They have many strong covalent bonds that need to be broken down to melt the solids
39
Why are not all of graphite’s electrons held in covalent bonds?
Has a layered structure, so not all electrons are held together by covalent bonds, these delocalised electrons are free to move and carry an electrical current
40
Why is graphite used in electrolysis?
It conducts electricity well and is cheap and not very reactive
41
Why is graphite a good lubricant?
The sheets in carbon atoms are held together by weak forces of attraction, these weak forces allow the layers to slide past each other, which makes graphite a good lubricant
42
What do atoms in a metallic element form?
Lattice
43
How many electrons do metals have in there outer shell?
1, 2 or 3
44
What is metallic bonding?
Electrostatic attraction between the positive metal ions and negative delocalised electrons
45
Do metals have high melting and boiling points?
Yes
46
Properties of metals?
- malleable - conduct electricity - conduct heat - high melting and boiling points
47
What is electrical conductivity?
Allowing electricity to pass through
48
What does a substance having a higher electrical conductivity mean?
They conduct electricity better than other substances
49
Why does the electrical conductivity of a metal increase?
When the number of delocalised electrons increase
50
Where are ionic bonds found?
In most compounds containing metal and non-metal atoms
51
How are ionic bonds formed?
The loss or gain of electrons to produce oppositely charged ions that attract one another
52
What is the structure of ionic bonds?
Billions of ions held together in a lattice structure
53
Properties of of ionic bonding?
- high melting/boiling points - many are soluble in water - conduct electricity when liquid but not when solid
54
Where are giant covalent bonds found?
In a few non-metal elements and some compounds of non-metals
55
When are covalent bonds formed?
When atoms share pairs of electrons
56
Properties of giant covalent bonds?
- high melting /boiling points - insoluble in water - most do not conduct electricity (except carbon as graphite)
57
Where are simple molecular bonds found?
In most non-metal elements and compounds
58
Properties of simple molecular bonds?
- low melting/boiling rates - insoluble in water - conduct electricity when solid or liquid
59
Where are metallic bonds found?
In all metals
60
What are metallic bonds?
Electrostatic attraction between positive metal ions and negative delocalised electrons

Chemistry (8 decks)

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