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Bonding & Properties Flashcards

1
Q

What are changes of state?

A

Physical changes that are reversible and do not change the chemical properties or makeup of substances involved

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2
Q

What does vaporisation include?

A

Evaporation and boiling

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3
Q

What is evaporation?

A

The change of liquid to gas, occuring only at the surface below boiling point

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4
Q

What is boiling?

A

Occurs at specific temperature when vapour pressure reaches external atmospheric pressure

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5
Q

Describe the relationship between temperature and energy during state changes.

A

Particles vibrate and gain kinetic energy as temp rises
All energy goes into breaking bonds - no increase in kinetic energy or temp
The particles move and gain kinetic energy
Substance is boiling, bonds are breaking so no increase in kinetic energy or temperature
Particles are moving around rapidly and increasing kinetic energy

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6
Q

Where are metals generally located on periodic table?

A

Left hand-side

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7
Q

Where are non-metals generally located on periodic table?

A

Right hand-side

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8
Q

What is ionic bonding?

A

Transfer of electrons from metallic element to non-metallic

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9
Q

How do electrons transfer in ionic bonding?

A

Metals lose electrons from outer shell to form cations
Non-metals gain electrons to form anions

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10
Q

Why do ionic compounds form?

A

Electrostatic attractions form between oppositely charged anions and cations

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11
Q

What is an ionic bond?

A

Electrostatic attraction formed in ionic compound
Non-directional - occurs in all directions

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12
Q

Why do ionic compounds have high melting points?

A

Very strong electrostatic attractions require lots of energy to overcome

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13
Q

How are ionic compounds arranged?

A

Giant ionic lattices

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14
Q

What is a lattice structure?

A

Ions are in regular repeating pattern so positive charges cancel negative

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15
Q

What charge does a lattice structure have?

A

Neutral - each ion attracted to all oppositely charged ions around it

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16
Q

What is covalent bonding?

A

The sharing of electrons between two non-metals

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17
Q

How are electrons shared in covalent bonding?

A

Electrostatic attraction between nuclei of two atoms and electrons of outer shells

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18
Q

How is a single covalent bond represented?

A

-

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19
Q

How is a double covalent bond represented?

A

=

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20
Q

How is a triple covalent bond represented?

A

≡

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21
Q

What type of diagrams are used to represent covalent bonding?

A

Dot and cross

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22
Q

What is a dot and cross diagram?

A

Diagrams that show the arrangement of outer-shell electrons in ionic and covalent compounds

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23
Q

Describe dot and cross diagrams.

A

Only outer electrons shown
Dots are used for electrons of one atom and crosses for the other
Electrons are shown in pairs
Even charge of ion shown using brackets
Charge written in top right coner

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24
Q

What is known as the “expanding the octet rule”?

A

Being able to accommodate more than 8 electrons in outer shell

25
What is meant by electron deficient?
Accommodating less than 8 electrons in outer shell
26
What is simple covalent bonding?
Two atoms sharing electrons
27
What is coordinate/dative covalent bonding?
Atoms that donate lone pair of electrons to form bond with electron-deficient atoms
28
How are metal atoms arranged?
Tightly packed in lattice structures
29
What are "delocalised electrons"?
Outer shell electrons that are free to move throughout metal lattice structure
30
Why do metal atoms in lattice structure become positively charged?
Outer electrons have dissociated
31
How do metal lattices remain in place?
Very strong electrostatic forces between positive metal ions and sea of delocalised electrons
32
How can covalent compounds be arranged?
Simple molecular Giant molecular lattices
33
Give examples of covalent compounds arranged in simple molecular form.
Iodine, Ice, Buckminsterfullerene
34
Give examples of covalent compounds arranged in giant molecular lattices.
Silicion oxide, Graphite, Diamond
35
What is formed if atoms are added to metal lattice?
Alloy
36
Why are alloys stronger than pure metals?
Other atoms stop layers of metal ions sliding over each other easily
37
How can the strength of metallic attraction be increased?
Increase number of delocalised electrons per metal atom Increase positive charges on ions Decrease size of ions
38
Why are metallic compounds malleable?
Metal layers can slide when force is applied Forces non-directional so metallic bonds can reform Lattice doesnt break and changes shape
39
Why are metallic compounds strong and hard?
Strong electrostatic forces between metal ions and delocalised electrons
40
Why can metals only conduct electricity in solid or liquid state?
Mobile electrons to freely move around and carry charge
41
Why are metals good thermal conductors?
Cations vibrate more vigorously as thermal energy increases Kinetic energy is transferred with collision Delocalised electrons carry increased kinetic energy and transfer it rapidly
42
Why do metals have high melting and boiling points?
Strong electrostatic forces of attraction between cations and delocalised electrons Large amounts of energy to overcome
43
Name the properties of metals.
Malleable Conduct electricity in solid and liquid state Thermal conductivity Strong + hard Insoluble in water High melting and boiling point
44
Name the properites of ionic structures.
Strong Brittle High melting and boiling point Soluble in water Conduct electricity when molten or in solution
45
Why are ionic compounds strong?
Strong electrostatic forces
46
Why do ionic compounds have high melting and boiling points?
Strong electrostatic forces between ions in lattice act in all directions Large amount of energy to overcome
47
Why are ionic compounds soluble in water?
Can form ion-dipole bonds
48
Why do ionic compounds only conduct electricity when molten or in solution?
Ions can move freely around and carry charge In fixed position in solid state
49
Name the properties of simple covalent lattice structures.
Low melting and boiling point Mostly insoluble in water Do not conduct electricity
50
Why do simple covalent lattices have low melting and boiling points?
Weak intermolecular forces Little energy required to break
51
When are simple covalent lattices soluble in water?
When polar and can form H bonds
52
Why don't simple covalent lattices conduct electricity?
No charged particles
53
Name the properties of giant covalent lattice structures.
Very high melting and boiling point Can be hard or soft Mostly insoluble in water Mostly do not conduct electricity
54
Why do giant covalent lattices have very high melting and boiling points?
Large number of covalent bonds link structure Large amount of energy required to break lattice
55
Why are some giant covalent lattices (graphite) soft?
Forces between carbon layers are weak
56
Why are some giant covalent lattices (diamond and silicon oxide) hard?
Difficult to break 3D network of strong covalent bonds
57
Why do some giant covalent lattices (graphite) conduct electricity?
Graphite has delocalised electrons between carbon layers which can carry charge
58
Why do some giant covalent lattices (diamond and silicon oxide) not conduct electricity?
All four outer electrons on every carbon atom involved in a covalent bond so no freely moving electrons

Save My Exams - Chem (20 decks)

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