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Bonding, structure and properties of matter Flashcards

(53 cards)

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1
Q

Describe ionic bonds (3 points)

A

-Takes place when metals and non-metals react by transferring electrons
-The atoms involved are oppositely charged particles (known as ions) in which electron transfer occurs
-The opposite charges attract through electrostatic forces

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2
Q

How are covalent bonds formed

A

non-metal atoms share pairs of electrons between each other

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3
Q

When are metallic bonds formed?

A

This type of bonding occurs in metals and metal alloys (mixtures of metals)

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4
Q

What is an ion?

A

An ion is an electrically charged atom or group of atoms formed by the loss or gain of electrons

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5
Q

Why do atoms lose or gain electrons?

A

To be stable and have a full outer shell of electrons

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6
Q

What are negative ions called?

A

Anions

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7
Q

What are positive ions called?

A

Cations

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8
Q

What ions do metals form?

A

Cations(+)

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9
Q

What ions do non-metals form?

A

Anions(-)

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10
Q

How are ionic compounds held together?

A

The positive and negative charges are held together by the strong electrostatic forces of attraction between oppositely charged ions

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11
Q

In what direction do electrostatic forces form?

A

In all directions

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12
Q

Describe the structure of an ionic compound?

A

The lattices formed by ionic compounds consist of a regular arrangement of alternating positive and negative ions in which the ions are tightly packed together

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13
Q

What allows solid ionic compounds to form regular shapes?

A

The lattice arrangement exists in three dimensions which allows solid ionic compounds to form regular shapes

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14
Q

Are covalent bonds strong?

A

Covalent bonds between atoms are very strong

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15
Q

When are molecules formed?

A

When two or more atoms are covalently bonded together, they form ‘molecules’

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16
Q

Describe inter molecular forces in a covalent molecule?

A

Weak inter molecular forces exist between individual molecules

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17
Q

Do simple covalent molecules conduct electricity? Why?

A

Simple covalent molecules do not conduct electricity as they do not contain free electrons

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18
Q

What is the difference between bonding in ionic vs covalent bonding?

A

In ionic bonds, electrons are completely transferred from one atom to another. In covalent bonding, electrons are shared between two atoms.

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19
Q

What are small covalent structures called?

A

These small molecules are known as simple covalent molecules

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20
Q

What are polymers?

A

Giant covalent structures

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21
Q

Name three substances with giant covalent structures

A

-Graphite
-Diamond
-Silicon dioxide

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22
Q

2 pros of dot and cross diagrams

Study These Flashcards
A

-shows the transfer of electrons
-shows which atom the electrons are coming from

23
Q

2 cons of dot and cross diagrams

Study These Flashcards
A

-Fails to illustrate the 3D arrangements of the atoms and electron shells
-Doesn’t indicate the relative sizes of the atoms

24
Q

2 pros of ball and stick model

Study These Flashcards
A

-Useful for illustrating the arrangement of atoms in 3D space
-Especially useful for visualizing the shape of a molecule

25
2 cons of ball and stick model
-Fails at indicating the movement of electrons -The atoms are placed far apart from each other, which in reality is not the case as the gaps between atoms are much smaller
26
2 pros of 2D model
-Displayed formulae are 2D representations and are basically simpler versions of the ball and stick model -Adequately indicate what atoms are in a molecule and how they are connected
27
2 cons of 2D model
-Fail to illustrate the relative sizes of the atoms and bonds -Cannot give you an idea of the shape of a molecule and what it looks like in 3D space
28
Describe the arrangement of atoms in pure metals
Metals consist of giant structures of atoms arranged in a regular pattern in a lattice
29
Are delocalised electrons transferred in metals
Delocalised electrons are not transferred as in ionic bonding, they are merely moving freely in the spaces in-between the nuclei of metal atoms.
30
What is an inter-conversion of state?
When matter changes from one state to another due to changes in temperature or pressure, the change is called an inter-conversion of state
31
Is an inter-conversion of state a physical or chemical change?
It is a physical change involving changes in the forces between the particles of the substances, the particles themselves remain the same, as do the chemical properties of the substance
32
What is sublimation?
gas to solid
33
What does particle theory explain?
Particle theory explains how matter changes state depending on the energy and forces present between the particles in the substance
34
What does the amount of energy needed to change from a solid to a liquid and from a liquid to a gas depend on?
The amount of energy needed to change from a solid to a liquid and from a liquid to a gas depends on the relative strength of the forces acting between the particles
35
Why is the amount of energy needed to change state for each substance different?
Since each substance contains different particles, then the amount of energy needed to induce a change of state is different for each individual substance
36
Why do particles gain more energy when they are heated?
When substances are heated, the particles absorb thermal energy which is converted into kinetic energy
37
How does melting occur?
Heating a solid causes its particles to vibrate more and as the temperature increases, they vibrate so much that the solid expands until the bonds break and the solid melts
38
How does Boiling occur
On further heating, the now liquid substance expands more and some particles at the surface gain sufficient energy to overcome the intermolecular forces and evaporate
39
What is latent heat?
While changing state, the temperature of the substance remains the same as the heat energy goes into breaking the bonds between the particles
40
Which diagram can be used to summarise latent heat?
Heating and cooling curve
41
Limitations of the particle model?(3)
-considers all particles to be solid,inelastic regardless of state -It doesn’t consider the difference caused by different particles, such as atoms, ions or molecules or mixtures of all three -The theory also fails to consider the intermolecular forces that exist between different particles in different substances
42
What does ⇌ show?
reversible
43
Physical properties of ionic compounds?(3)
-Soluble in water -hard + brittle -good insulators
44
Why do ionic compounds have high MP & BP points?
Ionic substances have high melting and boiling points due to the presence of strong electrostatic forces acting between the oppositely charged ions
45
When do ionic compounds conduct electricity?
Molten or liquid form
46
Why can't ionic compounds conduct electricity when solid?
They cannot conduct electricity in the solid state as the ions are in fixed positions within the lattice and are unable to move
47
Do small covalent molecules have a high or low BP?
Low boiling points due to weak intermolecular forces that require little energy to overcome
48
Can covalent compounds dissolve in water?
Most covalent compounds are insoluble in water as they tend to be non-polar but can dissolve in organic solvents
49
Can covalent molecules conduct electricity?
They are poor conductors of electricity as there are no free ions or electrons to carry the charge.
50
Are covalent molecules good insulators?
Most covalent compounds do not conduct at all in the solid state and are thus insulators
51
Where are intermolecular forces found?
Between molecules
52
Relationship between size of molecule and strength of intermolecular forces?
As the molecule increases in size the strength of the intermolecular forces increases
53
GOT UP to polymers

Chemistry (4 decks)

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