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Module 2: Foundations in chemistry > 2.2.2 Bonding and structure > Flashcards

2.2.2 Bonding and structure Flashcards

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1
Q

Blurt everything you know about 2 electron pairs.

A
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2
Q

Blurt everything you know about 3 electron pairs.

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3
Q

Blurt everything you know about 4 electron pairs.

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4
Q

Blurt everything you know about 5 electron pairs.

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5
Q

Blurt everything you know about 6 electron pairs.

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6
Q

How to work out the formula of an ionic compound.

A

Swap and drop meth

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7
Q

Blurt everything you know about ionic compounds

A
  • When negatively and positively charged ions bond (ionic bonding).
  • Most ionic compounds dissolve in water as they are polar and can attract + or - ions and break up the structure.
  • Conducts electricity when in molten or dissolved in solution as ions are free to move around
  • High melting points
    as there are strong electrostatic forces between oppositely charged ions. So lots of energy required to break these forces.
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8
Q

Blurt everything you know about covalent bonds give an example like ammonium.

A
  • Sharing of outer electrons in order to obtain a full shell.
  • Dative cov - One atom donates 2 electrons.
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9
Q

Draw the ionic bonding between Cl and Na,
Na and O
Mg and Cl
Al and F
(you may need more than one of an element for the ionic bonds). - easy

A
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10
Q

What and how becomes : polar molecule, and blurt everything you know about polar molecules, give examples

A
  • A big difference in electronegativity, makes the bond more polar.
  • As the charges don’t cancel out it is non-symmetrical
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11
Q

What happens when there’s a big difference in electronegativity

A
  • The compound will become more ionic.
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12
Q

How does a dipole-dipole get induced.

A
  • An induced dipole to dipole force occurs when a molecule is near another molecule. e.g bromine near ethene. in electrophilic addition. The ethene attracts on bromine and the electrons on the cov bond moves towards the second bromine.
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13
Q

Draw the bonding in O2 and N2

A
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14
Q

Hard : CO3 figure out the bonding and name the charge and OH?

A

The left-hand and bottom Oxygen atoms donate one dot each to form a single bond with the Carbon.

This leaves these two Oxygen atoms short of an electron each - this lack is made right by gaining two extra electrons (empty dots) and this is why it is CO32- rather than just CO3.

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15
Q

Draw CO2

A
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16
Q

What do we know about induced dipole to dipole forces, covalent bonds and a molecule

A
  • Induced dipole-dipole forces holds the molecule together. Say induced dipole-dipole forces between molecules.
  • Covalent bonds hold the 2 atoms together. Say covalent bonds between atoms in the exam
17
Q

Fill in the gaps:
1. The ____ the molecule or atom, the _____ forces you have, as you have a _____ cloud.
2. When we boil a liquid we break ______ not _____

A
  1. The bigger the molecule or atom, the induced dipole-dipole forces you have, as you have a larger electron cloud.
  2. When we boil a liquid we break weak induced dipole-dipole forces not covalent bonds
18
Q

Why do branched hydrocarbon bonds have lower boiling points and why do straight chain have higher boiling points.

A
  • Longer = more induced dipole-dipole forces = more energy needed to overcome these forces = boiling point increase.
  • Branched = can’t pack as closely together = less surface point of contact = weakness dipole-dipole forces = lower boiling point.
19
Q

Which molecules contain a hydrogen bond ?

A

When a hydrogen atom is bonded to either a nitrogen, oxygen or fluorine atom

20
Q

Draw a labelled diagram of the Hydrogen bonding in water 3 water molecules

A
21
Q

Draw a labelled diagram of the Hydrogen bonding in ammonia & ammonia

A
22
Q

Draw a labelled diagram of the Hydrogen bonding in ethanol & ethanol

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23
Q

Draw a labelled diagram of the Hydrogen bonding in ethanol & water

A
24
Q

Links between polar covalent bond, polarisation and electronegativity

A

Module 2: Foundations in chemistry (8 decks)

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