Revision(Units1&2) Flashcards

1
Q

Name 3 atoms with covalent network structure

A
  1. )Boron
  2. )Carbon
  3. )Silicon
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2
Q

Define Bonding Continuum

A

The sliding scale between ionic bonding and pure covalent bonding. Polar covalent bonding lies between these extremes.

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3
Q

Define Collision Theory

A

The theory that for a reaction to occur the reactant particles must come into contact with correct collision geometry

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4
Q

Define covalent radius and explain how it is measured.

A

The measure for the size of an atom.

It’s measured by half the nuclei of two covalently bonded atoms.

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5
Q

Define Dipole

A

An area with a higher concentration of negative or positive charge.

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6
Q

Fullerene

A

Molecules of pure carbon with the formula(C↓60 or C↓70).

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7
Q

Define ionic bond

A

Electrostatic attraction between positively and negatively charged ions.

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8
Q

Define Ionic radius

A

Measure of the size of an ion

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9
Q

At what state do at atoms have to be in, in order to measure their ionisation energy.

A

Gaseous state (g)

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10
Q

Define metallic bond

A

The electrostatic attraction between positively charged ions and delocalised electrons.

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11
Q

Define Viscosity.

A

A measure of how thick a liquid is.

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12
Q

Define Enthalpy change

A

The difference in energy, between the reactants and products.
Energy of Reactants - Energy of Products = ΔH enthalpy change = ΔH

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13
Q

What is a standard solution

A

Precisely/accurately know concentration of a solution.

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14
Q

How should a pipette be filled?

A

Fill a pipette to above the mark and then release liquid from the pipette until the bottom of the miniscus touches the mark.

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15
Q

Define Feedstock

A

A chemical from which other chemicals are manufactured.

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16
Q

How does the rate of reaction change when the equilibrium moves to the right?

A

Rate of forward reaction is increased.

17
Q

Why is deionised water used rather than that water in practicals?

A

Ions may be present in tap water.

Less ions will be in deionised water.

18
Q

What does polar covalent mean in terms of attraction to electrons

A

Both/all nuclei have the same attraction to electrons.

19
Q

Why do LDFs arise?

A

LDFs arise because temporary dipoles have been established.

20
Q

What is the notation of an enthalpy of combustion and is it exothermic or endothermic?

A
  1. )- ΔH

2. ) Exothermic