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Chemistry ATAR U1 > Bonding and Organic > Flashcards

Bonding and Organic Flashcards

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
How to name covalent molecular elements
Normal elements name
26
How to name covalent molecular compounds
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
How to name monoatomic bonds ionic compounds
Metal atom normal name - Can add roman numerals Non-Metal atoms add "ide" to end of name - Eg. Chlorine = Chloride
28
How to put together name for polyatomic bonds
1) Name of positve ion first 2) Name of negative ion second 3) Number of water molecules of crystallisation
29
How to name polyatomic bonds ionic compounds
Name cannot be predicted from formula
30
Writing formulae for ionic compounds
"swap and drop" method
31
How to name metallic bonds
Just the elemental name
32
How to draw metallic bond diagrams
No specific diagram (Eg. Lewis Dot diagram) Can just draw metal cations, with valence electrons floating around
33
How to write formulae for covalent bonds
Represents number & type of atoms present in molecule
34
What is hydrocarbons
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
What are alkanes / saturated hydrocarbons
Only carbon-carbon single bonds "Straight-Chain" of Carbon
36
What is molecular formula for alkanes / saturated hydrocarbons
Cn H2n+2 n(Hydrogens) = Double n(Carbons) + 2
37
What are alkenes / unsaturated hydrocarbons
Atleast one carbon-carbon double/triple bond Rest carbon-carbon single bonds
38
What is molecular formula for alkene / unsaturated hydrocarbons
Cn H2n n(Hydrogens) = Double n(Carbons)
39
What are physical properties of alkanes & alkenes
Low melting & boiling points, weak intermolecular forces Insoluble in polar substances, soluble in non-polar substances - Excellent solvents for oil-based products
40
What is structural formula and condensed structural formula
Structural formula shows all bonds in molecule Condensed structural formula shows atoms connected to each carbon atom
41
What are isomers
Molecules with same n(Carbon & Hydrogen) atoms, arranged differently
42
What are structural isomers
Same molecular formula, different arrangements of atoms in bonding
43
What are geometric isomers
Same molecular formula, different arrangement of atoms in space and restricted rotation
44
What are cis geometric isomers
On same side
45
What are trans geometric isomers
On different sides
46
What type of isomer does alkanes show
Structural isomers
47
What type of isomer does alkenes show
Structural isomers and geometric isomers
48
What is the process for naming alkanes
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
What is the process for naming alkenes
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
What is combustion
Combustion reactions with oxygen gas
51
What is complete combustion
Sufficient oxygen gas, water & carbon dioxide produced
52
What is incomplete combustion
Oxygen gas limited, water & carbon monoxide produced Exothermic reactions (Releases energy)
53
What are reactions with halogens
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
What is substitution reaction (Alkane or Benzene Reaction)
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
What is addition reaction (Alkane Reaction)
Double bond broken, new atoms bond to carbons either side of double bond Spontaneous, 1 product formed
56
What is hydrogenation (Adding hydrogens)
Metal catalysts present, alkenes react with hydrogen gas Alkane produced
57
What is halogenation (Adding halogens)
Room temperature, no catalysts Relatively fast, colour of halogen fading quickly Halogen adds across double bond, one halogen added to each carbon atom
58
What is adding hydrogen halides (Eg. HCl, HBr, HF, HI)
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
What is hydration (Addition of water)
Suitable catalyst present, alkenes react with water = Produces alcohols Water provides hydrogen to one carbon, hydroxyl (-OH) to other
60
What are nanomaterials
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
What is nanoscale
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
What are the risks of nanomaterials to health, safety, environment
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
What are the properties of nanomaterials different to bulk materials
Very small Bonded in rings of 5 or 6 carbons Made into ball or tube shape Structure changes as size changes
64
What are the pros and cons of nanoparticles in sunscreen
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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