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Chemistry Year 3/4 > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

What is a giant ionic lattice?

A

endlessly repeating 3D lattice of positive and negative ions which are closely packed arranged in an orderly manner and held in place together by strong ionic bonds!

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2
Q

What do ionic compounds have?

A

giant ionic lattice structure

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3
Q

What is a lattice?

A

arrangement of molecules/ions/atoms in regular pattern*

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4
Q

What makes an ionic compound have high melting point?

A

When there area strong forces of attraction between ions in a giant ionic lattice, larger amounts of energy is required to overcome these strong forces of attractions between oppositely charged ions in the giant ionic lattice so they have high melting boiling point

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5
Q

What does melting/boiling do to a compound?

A

Forces of attraction between ions are overcome causing ions to be free to move out of the ionic lattice strcture

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6
Q

Ionic compound properties?

A

high melting and boiling point ( more energy to overcome strong ionic bonds )
Non Volatile ( don’t evaporate in room temperature )
Exist as solid at room temperature
Brittle and solid are hard
Usually soluble in water
Usually INSOLUBLE in organic solvents ( ethanol turpentine petrol )
Large amount of energy required to overcome strong electrostatic forces of attractions betweeen anions and cations in compound during melting/boiling

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7
Q

How is electricity conducted?

A

when ions/electrons are able to move freely and act as mobile charged carriers = electricity can be conducted

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8
Q

Which state ionic compound has to be in to conduct electricity.

A

Aqueous molten state or liquid state. electricity andcan be conducted as ions can move freely throughout substance and behave as mobile charged carriers to conduct electricity
electricity andcan be conducted as ions can move freely throughout substance and behave as mobile charged carriers to conduct electricity

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9
Q

Can electricity conducted in solid?

A

since ions/electrons held in fixed positions ions are unable to move freely and act as mobile charged carriers to conduct electricity throughout a substance

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10
Q

Property of solid ionic compound and why its like that

A

Solid ionic compounds are hard because the giant ionic lattice structure formed has oppositely charged ions held in strong ionic bonds

brittle because stress applied on a solid ionic lattice causes sliding of layers of ions

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11
Q

How is lattice shattered?

A

ions of similar charges coming together hence the repulsion that occurs between like charge particles = shattering lattice

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12
Q

When covalent bond formed?

A

Formed when 2 or more atoms shares electrons in order to achieve table noble gas configuration

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13
Q

When does covalent bonding occur?

A

Between non-metals usually

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14
Q

Does covalent bonding occur between ions

A

There are only atoms no ions as in covalent bonds electrons aren’t lost or shared hence atoms stay electrically neutral during process of sharing atoms

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15
Q

What is valency

A

number of electrons that must be lost gained or shared in order for atom to achieve stable noble gas electronic configuration

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16
Q

What is the covalent bond?

A

Mutual electrostatic attraction between the shared paired of electrons and the nuclei of atoms

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17
Q

When is single covalent, double covalent, triple covalent bond formed?

A

Single covalent bond is when a pair of electrons are shared between 2 atoms
I
Double covalent bond is when 4 electrons are shared between 2 atoms

Triple covalent bond is of 6 electrons between 2 atoms

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18
Q

What is formed after covalent bond

A

When a covalent bond is formed between 2 atoms A MOLECULE FORMED

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19
Q

What makes a covalent molecules?

A

made from atoms of same or different elements

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20
Q

What do covalent substances exist as?

A

simple covalent molecules or giant covalent molecules

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21
Q

What defines a simple covalent molecule?

A

COUNTABLE number of atoms in a fixed ratio

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22
Q

What kind of bond do atoms in simple covalent molecules have?

A

Strong covalent bonds meaning there is strong mutual electrostatic attraction between the shared electrons and nuclei of atoms

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23
Q

Interatomic strength in simple covalent molecules?

A

It’s strong mutual forces of attraction between electrons of paired atoms and nuclei of atoms

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24
Q

What is the intermolecular strength of atoms in covalnet molecules which are simple?

A

MOLECULES IN COVALENT SUBSTANCES ARE HELD TOGETHER BY WEAK INTERMOLECULAR FORCES OF ATTRACTION

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25
What does weak intermolecular forces of attraction mean?
LOW MELTING BOILING POINT Of an ionic compound and Smaller amount of energy required to overcome weak INTERMOLECULAR FORCES OF ATTRACTION between molecules in covalent substance
26
Properties of simple covalent substances
Smaller amount of energy required to overcome weak INTERMOLECULAR FORCES OF ATTRACTION between molecules in covalent substance = LOW MELTING BOILING POINT Gasses/volatile liquids at room temp and pressure Insoluble in water, soluble in organic solvents ( ethanol turpentine petrol ) The larger the molecule THE INTERMOLECULAR FORCES OF ATTRACTION between molecules GETS STRONGER = melt/boil point INCREASES Doesn’t conduct electricity IN ANY STATE because there are no free mobile ions or electrons to move
27
Can simple covalent molecule ever conduct electricity?
HCL ( hydrogen chloride gas ) a simple covalent molecules form ions when dissolved in water forming aqueous solution hence the mobile ions can act as charged carriers to conduct electricity + liquid state allows ions to move freely
28
What is giant covalent molecules and what defines them?
Practically UNCOUNTABLE number of atoms with a network of strong covalent bonds and high melting boiling point
29
Example of giant covalnet molecule?
diamond and sand (aka silicon dioxide) giant molecules
30
What molecule is it if it has low melting boiling point
SIMPLE COVALENT MOLECULE
31
What molecule is it if molecule has high melting boiling point
giant covalent / ionic or metal structure
32
What is metallic bonding?
metals bonding with metals
33
What is a metallic bond?
refers to electrostatic forces of attraction between metal cations and sea of delocalised electrons
34
Do all metal compounds have a giant metallic lattice structure?
ONLY SOLID METALS HAVE IT
35
What is a giant metallic lattice structure?
giant structure of atoms arranged in endless 3D regular lattice pattern.
36
What does a metal form?
giant metallic lattice
37
What happens in a metal?
all the atoms lose their electrons and share them with all the other atoms in the metal
38
What happens when atoms lose their electrons to other atoms in a metal?
Now all atoms become metal cations and electrons are now free to move about = DELOCALISED
39
What makes a strong metal?
Strong forces of attraction between positive charges metal ions and negatively charged electrons holding everything together in a regular structure in metal = STRONG METAL
40
Why strong attraction force = strong solid?
strong forces of attraction between opposite charges = very strong bonds formed and solid substances at room temp are strong + with high melting boiling point
41
What happens to electrons in lead metal?
lead has a giant metallic lattice structure. The outermost electrons of lead atoms are delocalised into sea of electrons surrounding the orderly arranged lattice of positive lead ions
42
What happens to electrons in a giant metal lattice?
in a giant metallic lattice structure, metal atoms lose their valence electrons and become cations hence the remaining valence electrons no longer belonging to any metal atom become delocalised
43
Physical Properties of metal ( GHMD )
Good conductors of electricity and heat High melting boiling points Malleable Ductile
44
Why are metals good conductors of electricity and heat
due to presence of mobile delocalised electrons as they can act as mobile charge carrier to conduct electricity + THERMAL ENERGY
45
Why metals have high melting boiling points?
large amounts of energy is required to overcome strong electrostatic forces of attraction between cations and sea of delocalised electrons which have opposite charges
46
What does it mean metal is malleable and ductile?
Metal can be bent or flattened into sheets and can be drawn into wires without breaking.
47
What does it mean when a metal has more electrons?
*MORE ELECTRONS = STRONGER ATTRACTION BETWEEN CATIONS AND SEA OF DELOCALISED ELECTRONS = HIGHER MELTING/BOILING POINTS*
48
Downsides to pure metals?
Too soft ( malleable and ductile )
49
Why is it a downside that metals are soft?
Due to pure metals being soft, they have a regular lattice arrangement which causes layers of atoms to slide easily over one another when force applies (Sliding doesn’t disrupt metallic bonding!)
50
What are alloys?
mixture of a metal with one or more other elements
51
Properties of alloys?
1. Atoms in alloys have different sizes 2. Harder than pure metals
52
Why atoms in alloy different size and what does it mean?
Alloys are mixture of metal with one or more elements and atoms of different elements have different sizes. The diff sizes disrupts the regular lattice arrangement found in pure metals
53
Why allows harder than pure metals?
when lattice arrangement disrupted layers of atoms don’t slide over each other easily upon force applied = harder than pure metal
54
Do alloys have a lattice strcture?
No Since atoms in alloys are of different sizes there is irregular arrangement of atoms in the alloy disrupting the crystal lattice structure
55
What are the physical properties of alloys?
Makes metals harder and stronger Improve appearances of metals Lowers melting point of metals Metals more resistant to corrosion
56
Are pure metals malleable?
Pure metals have a regular structure = layers or atoms slide over one another upon pressure causing metals to be malleable
57
Are alloys malleable
No. different sized atoms disrupts metals regular strcture layers can no longer slide = alloy is harder than pure metal not malleable
58
Melting point ONLY MELT POINT of Giant Ionic Lattice? + room temp state + eg
Very high ( 700 to 300 degrees) and exist as solid at room temp Like sodium chloride
59
Simple molecular structure melting point ONLY and room temp state? + eg
Low melting point and usually exist as liquid or gas at room temperate Glucose and water
60
Giant metallic structure melt point + room temp state + eg
High melting point and exists as solid at room temperate usually like copper
61
What does malleable mean
Malleable = how easily can layers of atoms slide over each other
62
Describe bonding in covalent atoms?
Tell me if covalent bond between atom strong and if the intermolecular forces of attraction between molecules strong or not. Strong intermolecular = giant
63

Chemistry Year 3/4 (5 decks)

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