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Chemistry ATAR U1 > Bonding and Organic > Flashcards

Bonding and Organic Flashcards

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1
Q

What is metallic bonding and how is it made

A

Electrostatic attraction between positve cations and delocalised electrons
- Delocaliserd electrons free to move in 3-D lattice, attraction non-directional

Made through atoms losing electrons, becoming cations
- Electrons delocalise, where cations in fixed position, electrons aren’t

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2
Q

What is metallic bonding melting & boiling points

A

High melting & boiling points

Strong electrostatic attraction between cations & delocalised electrons
- More delocalised electrons = Stronger attraction
- Smaller cation = Stronger attraction

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3
Q

What is metallic bonding electrical conductivity

A

Good conductors of electricity

Delocalised electrons move towards positive electrode from negative electrode in circuit
- Number of electrons don’t change, carries current

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4
Q

What is metallic bonding thermal conductivity

A

Good conductors of heat

Heat energy picked up delocalised electrons, transferred through metal
- Energy absorbed by nucleus of cation, making it vibrate = Causes other nuclei to vibrate, conducting heat

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5
Q

What is metallic bonding malleability and ductility

A

Malleable and ductile

Force causes cations to roll over on eachother
- Layers of cations still held together by delocalised electrons between them
- Enough stress applied = Permanent change in position
- Therefore size of force required to deform bond = Large

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6
Q

What is ionic bonding and how is it made

A

Arrangement of positively & negatively charged ions in crystalline lattice (Positive & Negative)
- Strong electrostatic force of attraction between oppositely charged ions

Made through electron being transferred from metal to non-metal, so both can have full outer shell (Octet Rule)
- Anions & Cations form 3-D crystal lattice, held together by strong electrostatic forces

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7
Q

What is ionic bonding melting & boiling points

A

High melting & boiling points

Strength of electrostatic attraction between cations & anions large
- Large amount of energy needed to overcome attraction

  • Larger charge of ions = Stronger attraction
  • Smaller atoms = Stronger attraction
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8
Q

What is ionic bonding hardness & brittleness

A

Hard and brittle

Strength of electrostatic attraction between anions & cations large
- Strong force required to disrupt crystal lattice = Hard

When force large enough to disrupt lattice applied, brings like-charges next to eachother
- Like charges repel = Crystal shatters

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9
Q

What is ionic bonding electrical conductivity in ionic solids

A

Cannot conduct electricity

  • Ions in fixed positions, cannot move
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10
Q

What is ionic bonding electrical conductivity in ionic solutions / molten

A

Can conduct electricity

Ionic compound melt, ions free to move, cations & anions in compound can conduct electricity

Ionic compound dissolved, ionic bonds broken, can move freely in solution, conducting electricity

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11
Q

What is covalent molecular bonding

A

When valence electrons are shared between atoms, so atoms have full outer shell

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12
Q

How is covalent molecular bonds made

A

Non-Metallic atoms have high number of valence electrons, tend to share rather then transfer atoms
- Molecules formed more stable then regular atoms (Full outer shell)
- Positively charged nuclei of neighbouring atoms have attraction for shared electrons, keeps atoms held together in molecule (Electrostatic attraction)

  • Is direction bond, electrons aligned along axis between atoms that share electrons
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13
Q

What are the types of covalent bonds

A

Single covalent bond; Shares 1 pair of electrons (Eg. Cl2, H2)

Double covalent bonds; Shares 2 pairs of electrons (Eg. O2)

Can share up to 7 pairs of electrons
- 8th pair; Repulsive force so big, atom shatters
- One less valence electron = 1 more pair shared

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14
Q

What are covalent molecular bonding melting & boiling points

A

Low melting & boiling points

Covalent molecular solid melts/boils, breaks weak attractive forces with other molecules (Intermolecular forces)
- Requires little energy, easily overcome with low temperature
- Bonds between neutral molecules so weak, substances exist as gases or volatile liquids at room temperature

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15
Q

What are covalent molecular bonding electrical conductivity

A

Cannot conduct electricity

Electrons localised, not free to move
- Electrons shared, not transferred, so no charged ions

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16
Q

What are covalent molecular bonding hardness

A

Very soft, easily deformed, waxy appearance
Very little force required to push neutral molecules past eachother

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17
Q

What is covalent network bonding

A

Continuous array of covalently bonded atoms
- Ordered structure, can be crystal/lattice
- Large network of covalent bonds

Eg. Carbon atoms in diamond

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18
Q

What is covalent network bonding melting & boiling points

A

High melting & boiling points

Has many strong covalent bonds in a lattice which need to be broken

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19
Q

What is covalent network bonding electrical conductivity

A

Cannot conduct electricity

Electrons localised, not free to move
- Electrons shared, not transferred, so no charged ions

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20
Q

What is covalent network bonding hardness

A

Hard

In 3-D crystalline lattice, all covalent bonds held firmly in fixed position
- Strong covalent bonds between atoms (Intramolecular forces), making it hard

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21
Q

What are allotropes

A

Forms of a chemical element that exist in the same physical state (Different organisation of network)

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22
Q

What is diamond as an example of a carbon allotrope

A

Each carbon bonded to 4 other carbon atoms (Covalent network lattice)

No weak intermolecular forces, only strong covalent bonds in fixed positions (Intramolecular forces)

= Hard, non-conducting, high melting & boiling points, brittle

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23
Q

What is graphite as an example of a carbon allotrope

A

Each carbon bonded to 3 other carbon atoms, forms 2-D layers (Covalent layer lattice)

Strong covalent bonds between carbon atoms in layers, weak forces (Dispersion) between layers

= High melting & boiling points, hard in one direction but soft & slippery in another (Not brittle)

4th valence electron not bonded (Delocalised), can move through layer
= Electrical conductivity

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24
Q

What is fullerenes as an example of a carbon allotrope

A

Covalently bonded carbon in series of hexagons/pentagons, spherical/cylindrical shape

No delocalised electrons, atoms held in fixed positions, very few covalent bonds
= Soft, cannot conduct electricity, low melting point

Nanomaterial, each carbon bonded to 3 other carbons in ball or tube shape

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25
Q

How to name covalent molecular elements

A

Normal elements name

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26
Q

How to name covalent molecular compounds

A

Name of element closer to bottom or left side of periodic table written first
- Is normal element name

Second part of name obtained by adding ‘ide’ to end

If molecule contains more than one atom of same type, indicated by prefix
- “mono-“ = 1, “di-“ = 2, “tri-“ = 3, “tetra-“ = 4, “penta-“ = 5, “hexa-“ = 6
- “mono-“ cannot be used for first element

27
Q

How to name monoatomic bonds ionic compounds

A

Metal atom normal name
- Can add roman numerals

Non-Metal atoms add “ide” to end of name
- Eg. Chlorine = Chloride

28
Q

How to put together name for polyatomic bonds

A

1) Name of positve ion first
2) Name of negative ion second
3) Number of water molecules of crystallisation

29
Q

How to name polyatomic bonds ionic compounds

A

Name cannot be predicted from formula

30
Q

Writing formulae for ionic compounds

A

“swap and drop” method

31
Q

How to name metallic bonds

A

Just the elemental name

32
Q

How to draw metallic bond diagrams

A

No specific diagram (Eg. Lewis Dot diagram)

Can just draw metal cations, with valence electrons floating around

33
Q

How to write formulae for covalent bonds

A

Represents number & type of atoms present in molecule

34
Q

What is hydrocarbons

A

Covalent molecules only consisting of hydrogens & carbons

  • Combination of elements = Infinite combinations
  • As carbon has 4 valence electrons, each carbon forms 4 covalent bonds
  • Hydrogen forms 1 covalent bond
35
Q

What are alkanes / saturated hydrocarbons

A

Only carbon-carbon single bonds

“Straight-Chain” of Carbon

36
Q

What is molecular formula for alkanes / saturated hydrocarbons

A

Cn H2n+2
n(Hydrogens) = Double n(Carbons) + 2

37
Q

What are alkenes / unsaturated hydrocarbons

A

Atleast one carbon-carbon double/triple bond

Rest carbon-carbon single bonds

38
Q

What is molecular formula for alkene / unsaturated hydrocarbons

A

Cn H2n
n(Hydrogens) = Double n(Carbons)

39
Q

What are physical properties of alkanes & alkenes

A

Low melting & boiling points, weak intermolecular forces

Insoluble in polar substances, soluble in non-polar substances
- Excellent solvents for oil-based products

40
Q

What is structural formula and condensed structural formula

A

Structural formula shows all bonds in molecule

Condensed structural formula shows atoms connected to each carbon atom

41
Q

What are isomers

A

Molecules with same n(Carbon & Hydrogen) atoms, arranged differently

42
Q

What are structural isomers

A

Same molecular formula, different arrangements of atoms in bonding

43
Q

What are geometric isomers

A

Same molecular formula, different arrangement of atoms in space and restricted rotation

44
Q

What are cis geometric isomers

A

On same side

45
Q

What are trans geometric isomers

A

On different sides

46
Q

What type of isomer does alkanes show

A

Structural isomers

47
Q

What type of isomer does alkenes show

A

Structural isomers and geometric isomers

48
Q

What is the process for naming alkanes

A

1) Identify longest continuous carbon chain
- Give stem name and add “-ane” to end

2) If have branches, number carbons from end that gives side chain smallest numbers

3) Identify type & number of akyl groups attatched to chain

4) Place “number-name” at beginning of compounds name
- If two identical side hains, use prefixes to show how many, “position, position-name”

5) If different side chains, list in alphabetical order

Hyphens between number & word
Comma between two consecutive numbers

49
Q

What is the process for naming alkenes

A

1) Identify longest continuous carbon chain
- Give stem name and add “-ene” to end

2) Number carbon atoms in chain starting at end that gives lowest numbers to double bond

3) Identify position of double bond by lower number involved in bond
- Show number before “-ene”

4) List number & position of akyl side chains in beginning of compound’s name
- Alphabetical order
- If identical side chains, use prefixes to show how many there are

5) Identify if geometric isomers, if so;
- Add prefix “cis” or “trans” by which one it is

50
Q

What is combustion

A

Combustion reactions with oxygen gas

51
Q

What is complete combustion

A

Sufficient oxygen gas, water & carbon dioxide produced

52
Q

What is incomplete combustion

A

Oxygen gas limited, water & carbon monoxide produced

Exothermic reactions (Releases energy)

53
Q

What are reactions with halogens

A

Alkanes & alkenes react with halogens (Eg. F2, Cl2, Br2, I2)

Halogens bonded with hydrocarbons, uses prefixes
- “Fluoro”, “Chloro”, “Bromo”, “Ido”

Tells us if alkane or alkene

54
Q

What is substitution reaction (Alkane or Benzene Reaction)

A

Hydrogen replaced by halogen atom
Two products formed, 1 inorganic compound
Requires UV light to proceed (Not spontaneous)

Excess of halogen present after 1 substitution = More hydrogens can be substituted

55
Q

What is addition reaction (Alkane Reaction)

A

Double bond broken, new atoms bond to carbons either side of double bond

Spontaneous, 1 product formed

56
Q

What is hydrogenation (Adding hydrogens)

A

Metal catalysts present, alkenes react with hydrogen gas

Alkane produced

57
Q

What is halogenation (Adding halogens)

A

Room temperature, no catalysts

Relatively fast, colour of halogen fading quickly

Halogen adds across double bond, one halogen added to each carbon atom

58
Q

What is adding hydrogen halides (Eg. HCl, HBr, HF, HI)

A

React with alkenes, hydrogen added to one carbon, halogen added to other
- Non-Symmetrical alkenes, two different molecules, depends which atom each carbon bonds to

59
Q

What is hydration (Addition of water)

A

Suitable catalyst present, alkenes react with water = Produces alcohols

Water provides hydrogen to one carbon, hydroxyl (-OH) to other

60
Q

What are nanomaterials

A

Substances that contain particles in size range 1-100nm

Have specific properties relating to size of particles, which may differ to those of bulk material

61
Q

What is nanoscale

A

Structures betwene 1 and 100 nanometers across

Matter at nanoscale can be manipulated to create new materials, composites, devices

  • Different characteristics can provide commercially available products
  • Regulations developed, addresses new & existing nanoform materials
62
Q

What are the risks of nanomaterials to health, safety, environment

A

So small can travel through air, skin, into bloodstream

Particles interact with biomolecules = Unwanted chemiocal reactions

Other unknow risks, such as causing cancer

Small enough to penetrate lung cells

63
Q

What are the properties of nanomaterials different to bulk materials

A

Very small

Bonded in rings of 5 or 6 carbons

Made into ball or tube shape

Structure changes as size changes

64
Q

What are the pros and cons of nanoparticles in sunscreen

A

Zinc and titanium

Pros:
- Invisible sunscreen
- Reflects UV radiation

Cons:
- Unknown effects, such as causing cancers
- May go through skin and enter cells, harming them

Chemistry ATAR U1 (5 decks)

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