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Chemistry - S3 > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

3 types of bonding

A

Covalent , ionic , metallic

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2
Q

How do atoms become stable/have full outer electron shells

A
  1. Form ions (give away & accept electrons )
  2. Form covalent bonds with another atom (share a pair of electrons )
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3
Q

How is a covalent bond formed

A

A covalent bond forms when two non-metal atoms share a pair of electrons

held together by the electrostatic force of attraction between the positive nuclei of each atom and their negative electrons.

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4
Q

What does a covalent bond and what does it occur with

A

A covalent bond is a Strong force of attraction occurs between non metal atoms

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5
Q

How is a covalent discrete molecule form

A

(Most )Substance that form covalent bonds form individual or discrete molecules.

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6
Q

How to tell that is is a covalent discrete molecule

A

You can count the number of atoms & write its chemical formula.
They have a low melting point/boiling point ( below 500C )

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7
Q

What are covalent network structures

A

These are giant structures of nonmetal atoms held together by very strong covalent bonds , needing allot of energy to break them.

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8
Q

How to tell it’s a covalent network structure

A

Impossible/very hard to count exact number of atoms
High melting/boiling point ( above 500C )

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9
Q

Strong covalent bonds and weak intermolecular forces look like

A

Strong covalent bonds - black lines
Weak intermolecular forces - dashed lines

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10
Q

What chemical formula is buckminsterfullerene

A

C60

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11
Q

What are allotropes

A

Different forms of the same element

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12
Q

What is the most well known allotrope

A

Carbon

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13
Q

How does ionic bonding form

A

Forms between ions of metal & non metals

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14
Q

What kind of attraction does ionic bonding have

A

Very strong force of attraction

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15
Q

What is an ionic bond

A

Electrostatic attraction between oppositely charged ions

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16
Q

What makes up an ionic lattice( held up by what)

A

Ionic compounds held in place by strong ionic bonds

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17
Q

How to melt ionic bonds

A

Using allot of energy because of a high melting/boiling point

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18
Q

(Solubility) what did covalent and ionic substances dissolve

A

Covalent substances tend to dissolve other covalent substances
Ionic substances tend to dissolve other ionic substances

19
Q

What does it mean to be soluble

A

The ability to be dissolved

20
Q

Why is water a polar molecule

A

Because the electrons between oxygen and hydrogen atoms in water are not shared equally

21
Q

What does is mean that water is a polar molecule

A

One side of the molecule is slightly positive
other side of the molecule is slightly negative

22
Q

What can the polar molecule dissolve

A

Despite being covalent , water can dissolve ionic compounds but not covalent compounds

23
Q

Do ionic compounds conduct or not

A

They do conduct electricity when they are in solution or melted to form a liquid as the ions can move

24
Q

Do covalent compounds conduct electricity or not

A

They do not conduct electricity in any state

25
Q

What is the only acceptation to covalent compounds trying to conduct

A

Covalent compounds don’t conduct whereas carbon in the form of graphite even though it’s a covalent compound it does conduct

26
Q

What is metallic bonding

A

electrostatic attraction between positively charged
metal ions and a sea of delocalised (free) negative electrons

27
Q

What does it mean to be delocalised with metallic bonding

A

It means that they are free to move , allowing them to carry an electric charge through metallic structure

28
Q

What is electrolysis

A

It is the decomposition (break down ) of ionic compounds using electricity

29
Q

What ions are attached to what ( electrolysis)

A

Positive ions are attached to negative electrodes & negative ions are attached to positive electrodes

30
Q

What is an example of an electrolysis experiment

A

Copper chloride solution being broke down using electricity to form copper & chloride

31
Q

Where do covalent discrete molecules conduct electricity

A

They don’t conduct it in liquid , solid or solution

32
Q

Where do covalent network conduct electricity

A

They don’t conduct it in solution , solid or liquid

33
Q

Where do ionic bonds conduct electricity

A

Solid - they don’t conduct
Liquid - they conduct
Solution - they conduct

34
Q

Where do metallic bonds conduct electricity

A

Solid -they conduct
Liquid - they conduct
Solution- in soluble

35
Q

Most covalent substances don’t dissolve in water however what do they dissolve in

A

They do dissolve in oil.

36
Q

What is a molecule

A

A molecule is a group of atoms held together by covalent bonds.

37
Q

What is a diatomic molecule

A

Element Which is made of 2 atoms e.g H2 or N2

38
Q

What are balloon/petal diagrams used to show

A

how the outer electrons are shared between atoms to form covalent bonds.

39
Q

Examples of covalent network

A

diamond (carbon), sand (silicon
dioxide) and graphite (carbon).

40
Q

How to break an ionic lattice

A

Ionic compounds dissolve in water. When they dissolve in water the
lattice breaks up.

Solutions of ionic compounds can be broken down using a process called
electrolysis

41
Q

What is the only Liquid Metal ( metallic bonding)

A

Most metals are solids. Mercury is the only liquid metal.

42
Q

Why can metals conduct electricity

A

As electrons can move from metal ion to metal ion, metals conduct
electricity.

43
Q

What is a covalent discrete molecule

A

A covalent molecule in which the Intermolecular forces are really weak

Chemistry - S3 (4 decks)

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