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Higher chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

First ionisation energy

A

the energy required to remove one mole of electrons from one mole of gaseous atoms

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2
Q

What type of reaction is ionisation energy

A

endothermic (positive) as it requires energy to break electrostatic attraction.

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3
Q

Trend in ionisation energy across the period

A

increases- increased nuclear charge, more energy required to remove electrons.

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4
Q

trend in ionisation energy down a group

A

decreases- increasing electron shells, inner shells shield outer shells from nuclear charge meaning less energy required to remove electron.

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5
Q

Why might the second ionisition energy of an atom be much higher than the first?

A

because an electron is being removed from a full, stable shell that is closer to the nucleus

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6
Q

Definition of covalent radii

A

half the distance between the nuclei of two covalenty bonded atoms

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7
Q

Trend in covalent radii across the period

A

decrease- increasing nuclear charge which pulls electron shells more closer to the nucleus

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8
Q

Trend in covalent radii down a group

A

increases- increasing electron shells

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9
Q

Definition of electronegativity

A

the measure of attraction an atom involved in a bond has for the electrons in that bond

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10
Q

Trend in electronegativity across the period

A

increases- nuclear charge increases which creates a stronger electrostatic attraction, electrons held more tightly

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11
Q

Trend in electronegativity down a group

A

decreases- increasing electron shells. inner shells shield outer shells from nuclear charge, electrons further from nucleus

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12
Q

What is metalic bonding?

A

positive metal ions surrounded by a sea of delocalised electrons

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13
Q

What are the properties of metalic bonding?

A
  • lattice= hight mp and bp.
  • can conduct due to delocalised electrons
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14
Q

What is covalent bonding?

A

shared pair of electrons between atoms.

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15
Q

What are the properties of covalent molecular bonding?

A
  • discrete= low mp and bp
  • weak intermolecular forces
  • doesn’t conduct
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16
Q

What are the properties of covalent network bonding?

A
  • network= high mp and bp
  • strong covalent bonds
  • doesn’t conduct (except graphite)
17
Q

What is ionic bonding?

A

attraction between positive and negative ions

18
Q

What are the properties of ionic bonding?

A
  • lattice= high mp and bp
  • free ions
  • conduct when molten or in solution
19
Q

What is intramolecular bonding?

A

forces within the molecule (covalent, ionic etc)

20
Q

What is intermolecular bonding?

A

forces between molecules (LDF, pd-pd, hydrogen)

21
Q

What bonding is there in the first 20 elements?

A

COVALENT MOLECULAR= diatomic (gas), P4, S8, fullerencs (C60)
METALIC= group 1 (except H), group 2, aluminium.
MONATOMIC= group 8/0
COVALENT NETWORK= Boron, Carbin, Silicon

22
Q

LDF properties

A

-weakest
- Arise due to an uneven distribution of electrons, causing temorary dipoles, then causing induced dipoles in neighbouring atoms
- more electrons= stronger LDF

23
Q

List the types if intermolecular bonding from weakest to strongest

A

LDF, Pd-Pd, Hydrogen

24
Q

Pd-Pd properties

A
  • stronger than LDF’s
  • Arises when theres a difference in electronegativity
  • can also arise due to an uneven structure
  • Higher mp and bp
25
Q

Hydrogen bonding properties

A
  • strongest
  • Arises when H is bonded to N, O, or F.
  • creates a stronger pd-pd than before
26
Q

What are the physical properties relation to intermolecular bonding?

A
  1. Melting and boiling points: water has a much higher bp due to hydrogen bonding.
  2. Viscosity (thickness of a liquid): higher mass= more viscous (thicker), higher amount of hydrogen bonds in a molecule the greater the viscosity.
  3. miscibility: like dissolves like
  4. solubility: like dissolves like
27
Q

What is non-polar?

A

BONDS= no difference in electronegativity
PHYSICAL= symmetrical (cancels out polarity)

28
Q

What is polar?

A

BONDS= difference in electronegativity
PHYSICAL= aesymmetrical

29
Q

What is a polar covalent bond?

A

when a shared pair of electrons in a covalent bond are not shared equally.

30
Q

What is pure covalent bonding?

A

when a shared pair of electrons are shared equally

31
Q

What does ionic character mean

A

increasing ionic character= increasing polarity

32
Q

What is an oxidising agent?

A

A substance which is being reduced, strong oxidising agents-bottom left

33
Q

What is a reducing agent?

A

a substance which is being oxidised, strong reducing agent top right

34
Q

What is oxidisation?

A
  • Loss of electrons
  • gain of oxygen
  • Loss of hydrogen
35
Q

What is reduction?

A
  • Gain of electrons
  • Loss of oxygen
  • Gain of hydrogen
36
Q

steps of balancing ion electron equations

A
  1. balance elements
  2. balance oxygens (add water on opposite side)
  3. balance hydrogen to balance h (add H ions on opposite side from water)
  4. add electrons to balance charge
37
Q

What are the compounds for reducing and oxidising agents?

A

REDUCING= carbon monoxide
OXIDISING= dichromate, permanganate, hydrogen peroxide

38
Q

What are the everyday uses of oxidising agents?

A

Can kill fungi and bacteria

39
Q

what is a fullerene?

A
  • a form of carbon
  • exist as discrete covalent molecular
  • cannot conduct

Higher chemistry (3 decks)

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