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Chemistry > C2-bonding,structure And Properties Of Matter > Flashcards

C2-bonding,structure And Properties Of Matter Flashcards

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1
Q

What is ionic bonding

A

Ionic bonding is the electrostatic attraction between oppositely charged ions (metals and non metals) by the transfer of electrons

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2
Q

What happens in group down as you go down

A

It gets more reactive

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3
Q

Define an ion

A

A charger particle

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4
Q

What charge do metals have
What charge do non metals have

A

Positive because they are donating negative electrons

Negative because they Are receiving negative electrons

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5
Q

What does a giant ionic lattice consist of

A

Positive metal ions
Negative non metal ions
Regular repeating pattern of alternative ions

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6
Q

What is the chemical name for table salt

A

Sodium chloride (NaCl)

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7
Q

Salt can dissolve in solvents such as water. What does this tell us about salt

A

That it is a soluble solute meaning it can dissolve in a solvent creating a solution

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8
Q

Define electricity

A

Electricity is the flow of electrons

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9
Q

Can NaCl (s) conduct electricity?

A

No because all of the ions are bonded together and there are no free moving ions/electrons to carry the charge around the structure. Electricity is the flow of electrons.

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10
Q

What does aqueous mean?

A

Dissolved in a solvent

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11
Q

Can NaCl (l) (aq) conduct electricity?

A

Yes because water breaks the bonds between the ions (intermolecular forces) meaning they are free to move around the structure and carry charge. Electricity is the flow of electrons/ions

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12
Q

Describe the structure of sodium chlorides structure (ionic lattice)

A

Consists of positive metal ions and negative nonmetal ions that are held in place by electrostatic attraction. It has a regular repeating pattern of alternative ions. The electrons from sodium have been donated to chlorine. When reacted together. It is a giant ionic lattice structure.Na+ Cl-

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13
Q

Ionic bonds share or transfer electrons?
Covalent bonds share or transfer electrons?

A

Transfer
Share

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14
Q

Ionoic bonds exist between?
Covalent bonds exist between?

A

Metals and non metals
Non metals and non metals

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15
Q

When can ionic compounds conduct electricity

A

When dissolved or melted
(Aqueous or molten)

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16
Q

Why don’t covalent bonds conduct electricity

A

There are no free ions. No electrons move because they are all used up in bonding.

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17
Q

Intermolecular forces

A

Occuring amongst or between molecules.
Weak
Van der walls
Opposite of covalent bonding

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18
Q

Intramolecular forces

A

Bonds inside a molecule (covalent bond)
Strong (cannot be broken)

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19
Q

Name some simple covalent molecules

A

Hydrogen H(2). Gas
Sulfar S(8). Solid
Water H(2)O. Liquid
Carbon dioxide CO(2). Gas

20
Q

Small molecules

A

Substances that consist of small molecules are usually gasses or liquids. Relatively low melting and boiling point.

21
Q

What is the chemical name for sand

A

Silicone dioxide

22
Q

What are delocalised electrons

A

Electrons that can move

23
Q

Define covalent bonding

A

Where 2 atoms share one or more pair of electrons. Sharing helps then achieve a full outer shell which stabilises them. Between non metal and non metal.

24
Q

Giant structures

A

Very high melting and boiling points
Most compounds are insoluble with water
Compounds can be hard or soft
Most compounds do not conduct electricity however some do
Large number of covalent bonds linking the whole structure

25
Q

How are particles arranged in a solid

A

Arranged close together im a fixed pattern.They vibrate in place but do not move freely.The strong forces between the particles keep them tightly packed making them stable.
Definite shape and definite volume

26
Q

How are particles arranged in a liquid

A

Arranged close together but not in a fixed position. They can move past each other which allows them to flow and take the shape of their container. The forces between particles are weaker than in solids. Have definite volume but not definite shape

27
Q

How are particles arranged in a gas

A

Arranged far apart for each other and can move freely in all directions.Have lots of energy allowing them to overcome any forces between them. No definite shape or definite volume. Expand to fill container.

28
Q

Define metallic bonding

A

Metallic bonds are the attraction between the positive metal ions and the sea of delocalised negative electrons

29
Q

What does malleable ductile and sonorous mean

A

Malleable- can be shaped into different shapes
Ductile-can be shaped into wires
Sonorous-makes a ringing sound when hit

30
Q

Define alloy and give examples of it

A

An alloy is a mixture of two or more elements where at least one is a metal. Stainless steel, steel, bronze

31
Q

Define melting point

A

The temperature at which a solid starts to turn into a liquid because of the energy it is given

32
Q

Define boiling point

A

The temperature at which a liquid starts to turn into a gas because of the energy it is given

33
Q

Write all key words to do with changes of states of matter

A

S-L=melting
L-S=freezing
L-G=evaporating
G-L=condensing
G-S=deposition (frost)
S-G=sublimation (dry ice)

34
Q

Define polymer

A

A very large molecule made from many repeating units called monomers

35
Q

What are polymers made from and examples of some

A

Polymers are made cor alkenes (ethene propene butene)

Polyester, polystyrene, polyvinyl chloride, polyvinyl astatate)

36
Q

How to turn ethene into monomer and polymer

H. H
C=C
H. H

A

Monomer- break the carbon double bond and put it at each side of carbon then put square brackets around it and add an n next to it small. (Make sure the lines go outside brackets)

Polymer-break the carbon double bond and out it at each side of carbon then repeat this a few times and draw them all next to each other so 2 bonds are joined together at each side

37
Q

What can nanoparticles be used as?

A

Catalysts, nano-medicine and tint electrical circuits

38
Q

Define allotrope

A

Different forms of the same element where atoms are arranged in a different way

39
Q

List properties of graphite

A

Strong covalent bonds
Smaller covalent structure
Three atoms,layers
Low melting point
Held together by weak intermolecular bond that dont require alot of energy to break
Conducts electricity, free moving electrons

40
Q

List properties of diamond

A

Strong covalent bonds
Giant covalent structure
Four atoms, tetrahedral structure
High melting point
Held together by strong covalent bonds that require lots of energy to break
Dosent conduct electricity

41
Q

What are the 4 allotropes of carbon

A

Fullerene, diamond, graphite, graphene
(Medicine) (drills) (pencils,lubricant)

42
Q

Why is graphite soft

A

Layers because weak intermolecular forces allowing layers to slide off eachother

43
Q

What is nanoscience

A

Refers to structures that are 1-100nm in size.
.it gives antibacterial,antiviral and anti fungal properties to things such as silver atoms.
.can kill pathogens and reduce bacteria that can cause food poisoning
.silicone dioxide can be used in armour because it is strong snd lightweight ideal for protection and ease wearing
.sports equipment stronger and lightweight.layer slows down the escape of air so ball dosent lose pressure as quick.
.Nanoparticles stronger and harder than normal metals bc inserted into layers of metals
.zinc oxide suncream. Absorbs radiation such as ultraviolet that cause skin damage.
.pass thru skin can damage cells eg skin bone
.can cause harm if used inside or on human body. Spread in air or water causing damage to other life

44
Q

How does graphite conduct electteicity

A

Each carbon atom is bonded to three carbon atoms. Leaving one delocalised electron which can carry charge thru the structure.

45
Q

How does sodium chloride conduct electricity

A

Sodium chloride, only conducts electricity when it is molten or in an aqueous solution. Therefore, the ions are free to move. This means that they can carry charge through the structure.

Chemistry (3 decks)

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