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Chem (SQA accurate) Knowledge > Unit 3 > Flashcards

Unit 3 Flashcards

(45 cards)

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1
Q

What types of substances usually join together to form ionic compounds?

A

A metal and a non-metal

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2
Q

Describe ionic bonding.

A

An electrostatic force of attraction between oppositely charged ions.

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3
Q
  1. What can be said about the strength of ionic bonds?
A

Ionic bonds are strong

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4
Q
  1. Why do atoms gain or lose electrons?
A

To gain full outer energy levels

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5
Q
  1. What always happens when metal atoms form ions?
A

They form positive ions

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6
Q
  1. How do you work out how many electrons a metal loses when it forms an ion?
A

You can work out how many electrons a metal loses by using its group number, this tells you how many electrons are on its outer shell, therefore how many electrons it needs to lose

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7
Q
  1. What happens to non-metal atoms when they form ions?
A

They gain electrons to form negative ions

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8
Q
  1. How do you work out how many electrons a non-metal atom gains when it forms an ion?
A

You can work out how many electrons a non-metal gains by using its group number, this tells you how many electrons are on its outer shell, then work out how many more it needs to gain a full outer energy level.

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9
Q

(a) Know how to write nuclide notation for ions. E.g. how would you write the nuclide notation for a chloride ion with mass number 35?

(b) Know how to work out the number of protons, neutrons and electrons when given the nuclide notation of an ion.

A

35
Cl-
17

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10
Q
  1. What type of substances have metallic bonding?
A

Metals

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11
Q
  1. Describe metallic bonding (with the aid of an annotated diagram).
A

Electrostatic force of attraction between positive metal ions and delocalised electrons

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12
Q
  1. What can be said about the strength of the metallic bond?
A

Metallic bonds are strong

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13
Q
  1. What type of elements usually form covalent compounds?
A

Non-metals

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14
Q
  1. What is a covalent bond?
A

A shared pair of electrons between two non-metal atoms.

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15
Q

What holds the atoms together in covalent bonding?

Draw a diagram to represent a covalent bond in a hydrogen molecule, H2.

A

The atoms are held together by the electrostatic force of attraction between the positive nuclei and shared pair of electrons.

https://docs.google.com/document/d/1KxSxHupC9-wwz7iCN8x6jaGNmWuZ0WIG8WW2AM6Tbm0/edit?tab=t.0

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16
Q

Be able to draw diagrams to show how the outer electrons are shared in elements and compounds to form covalent bonds.

i.e. Draw a diagram showing the outer electrons in a molecule of
(a) Chlorine
(b) Oxygen
(c) Nitrogen

A

https://docs.google.com/document/d/1KxSxHupC9-wwz7iCN8x6jaGNmWuZ0WIG8WW2AM6Tbm0/edit?tab=t.0

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17
Q
  1. What is the formula for an oxygen molecule? How many bonds are there between atoms?
A

O2
There are two covalent bonds (double covalent bond)

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18
Q
  1. What is the formula for a nitrogen molecule? How many bonds are there between atoms?
A

N2
There are three covalent bonds (triple covalent bond)

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19
Q
  1. What is a molecule?
Study These Flashcards
A

A group (small number) of atoms held together by covalent bonds

20
Q
  1. What is a diatomic molecule?
Study These Flashcards
A

A molecule that consists of two atoms

21
Q
  1. What are the 7 elements that exist as diatomic molecules?
Study These Flashcards
A

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromie
Iodine

22
Q
  1. What shape are diatomic molecules?
23
Q
  1. Name and draw the shape of some 3 atom molecules (containing 2 bonds), such as water.
Study These Flashcards
A

Water has an angular shape

https://docs.google.com/document/d/1KxSxHupC9-wwz7iCN8x6jaGNmWuZ0WIG8WW2AM6Tbm0/edit?tab=t.0

24
Q

What is the shape of 4 atom molecules (containing 3 bonds) such as nitrogen hydride (ammonia)?
Draw this molecule in 3D.

Study These Flashcards
A

Ammonia has a trigonal pyramidal shape

25
What is the shape of 5 atom molecules (containing 4 bonds) such as carbon hydride (methane)? Draw this molecule in 3D.
Methane has a tetrahedral shape
26
26. What is meant by a discrete molecular substance?
A covalent substance where the molecules exist separately
27
What term is used to describe bonds between molecules?
Intermolecular forces are weak
28
29. What does the formula of discrete covalent substances tell you?
The number of atoms in the molecule
29
31. Name 2 elements with a covalent network structure.
Carbon (diamond and graphite) Silicon
30
Name 2 compounds with a covalent network structure.
Silicon dioxide Silicon carbide
31
What type of structure do ionic compounds have? Draw the structure for sodium chloride.
Ionic crystal lattice
32
What information do you get from the formulae of an ionic compounds? e.g. MgCl2
The ratio of each ion present in the lattice
33
35. What is an electric current?
A flow of charged particles
34
36. What charged particles can carry a current?
Ions or delocalised electrons
35
37. Why do metals and carbon (graphite) conduct electricity?
They both have delocalised electrons (electrons which are free to move)
36
38. Why do covalent compounds not conduct electricity?
There are no charged particles free to move
37
39. In what state will ionic compounds conduct?
Solution (dissolved in water) or molten
38
40. Why do ionic compounds conduct when dissolved or molten but not when solid?
Ionic substances conduct when molten or in solution as the ions are free to move, whilst when solid the ions are fixed (cannot move)
39
41. Why do metals have high melting and boiling points?
To melt or boil a metal, you need to break the metallic bonds which are strong. This requires a lot of energy.
40
42. Why do ionic compounds have high melting and boiling points?
To melt or boil an ionic compound, you need to break the ionic bonds which are strong. This requires a lot of energy.
41
43. Why do covalent network structures have high melting and boiling points?
To melt or boil a covalent network, you need to break the covalent bonds which are strong. This requires a lot of energy.
42
44. Why do discrete covalent molecular substances have low melting and boiling points?
To melt or boil a covalent molecule, you need to break the weak intermolecular forces which are between molecules. This does not require a lot of energy.
43
45. What can be said of the solubility of ionic substances in water?
Generally soluble (check the Data Booklet)
44
Metals and non-metals usually form?
Ionic bonds
45
Two (or more) different non-metals usually form?
Covalent bonds

Chem (SQA accurate) Knowledge (9 decks)

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