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Chemistry : Unit 1 > Bonding > Flashcards

Bonding Flashcards

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0
Q

Ionic Bonding forms between…

A

A metal and non-metal.

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1
Q

Ionic Bonding is…

A

The electrostatic forces of attraction between the oppositely charged ions.

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2
Q

In Ionic Bonding, electrons are…

A

Transferred.

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3
Q

In Ionic Bonding, metals…

A

Lose electrons to form positive ions (cations).

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4
Q

In Ionic Bonding, non-metals…

A

Gain electrons to form negative ions (anions).

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5
Q

Opposite ions..

A

Attract.

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6
Q

Like ions…

A

Repel.

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7
Q

Why do Ionic compounds have high boiling and melting points?

A

Ionic compounds have strong electrostatic forces of attraction between the oppositely charged ions which requires a lot of energy to break the bonds.

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8
Q

Why don’t Ionic compounds conduct electricity when solid?

A

Ions are held together strongly and therefore can’t move.

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9
Q

Why can Ionic compounds conduct electricity when molten or dissolved in water?

A

The ions are free to move and carry the current = delocalised electrons.

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10
Q

Why are Ionic compounds described as being hard and brittle?

A

Ions cannot move or slip over each other easily.

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11
Q

Are Ionic compounds soluble or insoluble in water?

A

Soluble.

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12
Q

If a non-metal gains two electrons, what charge will it have?

A

2-

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13
Q

If a metal loses one electron, what charge will it have?

A

1+

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14
Q

What is Covalent Bond?

A

A shared pair of electrons.

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15
Q

A Covalent Bond forms between…

A

Two non-metals.

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16
Q

In Covalent Bonding, atoms…

A

Share electrons.

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17
Q

Why do atoms share electrons in Covalent Bonding?

A

To get to the nearest noble gas electronic configuration.

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18
Q

Fluorine reacts with Bromine to form liquid Bromine Trifluoride (BrF3). State the type of bond between Br and F in BrF3 and state how this bond is formed.

A

Type of bond: Covalent.

How bond is formed: Shared pair of electrons.

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19
Q

Name the type of bonding in Sodium Chloride.

A

Ionic Bonding.

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20
Q

Suggest the type of crystal shown by OF2.

A

Simple Molecular (Simple Covalent)

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21
Q

Are Simple Covalent Compounds/Molecular Crystals usually solid, liquid or gases?

A

They are usually gases or volatile liquids.

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22
Q

What are the three types of Intermolecular Forces?

A

Van der Waals
Permanent dipole-dipole
Hydrogen Bonding

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23
Q

What is meant by the term Electronegativity?

A

The ability of an atom to withdraw (attract) electrons from a covalent bond to itself.

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24
Q

Most electronegative element?

A

Fluorine.

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25
Q

What are the four most electronegative atoms?

A

Fluorine, Oxygen, Nitrogen and Chlorine.

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26
Q

Why does electronegativity INCREASE across a period?

A

The nuclear charge increases, shielding stays the same and electrons become more strongly attracted to the atom.

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27
Q

Why does electronegativity DECREASE down a group?

A

The distance between the nucleus and the outer electrons increases, shielding increases and electrons become less attracted to the atom.

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28
Q

Why can’t Noble Gases be described as electronegative?

A

They do not form bonds.

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29
Q

What is the strongest Intermolecular Force?

A

Hydrogen Bonding.

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30
Q

Van der Waals forces become stronger as…

A

The number of electrons increase and when there is a greater surface area.

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31
Q

Hydrogen bonds will form if…

A
  • A molecule contains a Hydrogen atom covalently bonded to a Nitrogen, Oxygen or Fluorine atom.
  • There is a lone pair of electrons on the N, O or F atom.
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32
Q

Hydrogen Bonding is represented by…

A

A dashed line that ends at a lone pair of electrons on the electronegative element N, O or F.

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33
Q

Lone pair / Lone pair bond angles are..

A

The biggest.

34
Q

Bonding pair / Bonding pair bond angles are…

A

The smallest.

35
Q

Lone pair / Bonding pair bond angles are…

A

The second biggest.

36
Q

What is a lone pair of electrons?

A

Unshared electrons.

37
Q

3 bonded pairs. No lone pairs. Angle: 120.

A

Trigonal Planar.

38
Q

Octahedral?

A

6 bonding pairs. No lone pairs. Angle: 90.

39
Q

5 bonded pairs. No lone pairs. Angle: 90 and 120.

A

Trigonal Bipyramidal.

40
Q

Square Planar?

A

4 bonded pairs. 2 lone pairs. Angle: 90.

41
Q

T-Shaped?

A

3 bonded pairs. 2 lone pairs. Angle: 90.

42
Q

3 bonded pairs. 1 lone pair. Angle: 107.

A

Trigonal Pyramidal.

43
Q

Linear?

A

2 bonded pairs. No lone pairs. Angle: 180.

44
Q

2 bonded pairs. 2 lone pairs. Angle: 104.5.

A

Bent Planar.

45
Q

Tetrahedral?

A

4 bonded pairs. No lone pairs. Angle: 109.5.

46
Q

Shape of PCl3?

A

Trigonal Pyramidal.

47
Q

Shape of CO2?

A

Linear.

48
Q

Shape of NH4+?

A

Tetrahedral.

49
Q

Shape of CO3(2-)?

A

Trigonal Planar.

50
Q

The four types of Crystals are…

A

1 - Ionic
2 - Metallic
3 - Molecular (Simple Covalent)
4 - Macromolecular (Giant Covalent)

51
Q

Two main examples of Macromolecular Crystals…

A
  • Diamond

* Graphite

52
Q

A Co-Ordinate / Dative Bond forms when…

A

The shared pair of electrons in the covalent bond are donated from one atom.

53
Q

For a co-ordinate / dative bond to form…

A
  • One atom must have a lone pair of electrons.

* The other atom must have a vacant orbital (empty orbital).

54
Q

A dative covalent bond is represented by…

A

A short arrow from the atom/donor providing both electrons to the atom/acceptor of the electron pair.

55
Q

NHF2 + BF3 > F2HNBF3

State the type of bond formed between the an atom and the B atom in F2HNBF3. Explain how this bond is formed.

A

Type of Bond: Dative/Co-Ordinate Bonding.

How the bond is formed: The lone pair of electrons on the Nitrogen are donated to Boron (empty orbital).

56
Q

A Metallic Bond is…

A

The electrostatic force of attraction between the positive metal ions and the delocalised electrons.

57
Q

3 main factors that effect the strength of a metallic bond are…

A

1 - The number of outer delocalised electrons.
2 - Size of the ion. (Smaller the ion, stronger the bond)
3 - Number of protons / nuclear charge.

58
Q

Describe the structure of a Magnesium Crystal.

A

A lattice of positive ions surrounded by a sea of delocalised electrons.

59
Q

Explain why metals are usually malleable and ductile.

A

Ions can slide over one another and the delocalised electrons prevent repulsion between the positive ions.

60
Q

How does a metal conduct electricity?

A

When solid and molten. Electrons are delocalised therefore they can move through the structure and carry the charge.

61
Q

Are Metallic Bonds soluble or insoluble in water?

A

Insoluble.

62
Q

An Aluminium Chloride molecule reacts with a Chloride ion to form the AlCl4(-) ion. Name the type of bond formed in this reaction. Explain how this type of bond is formed in the AlCl4(-) ion.

A

Type of Bond: Dative.

Explanation: The lone pair of electrons on the Cl- are donated to the empty orbital in AlCl3.

63
Q

State the type of Crystal structure for each of Iodine and Graphite.

A

Iodine - Simple Molecular.

Graphite - Macromolecular.

64
Q

Carbon in Graphite is covalently bonded to…

A

3 other Carbon atoms.

65
Q

Describe the structure of and bonding in Graphite and explain why the melting point of Graphite is very high.

A

Graphite is arranged in layers of Carbon atoms (hexagons). Each Carbon is covalently bonded to 3 other Carbon atoms. Graphite has a very high melting point because of the strong covalent bonds in the macromolecular structure. It requires a lot of energy to break the strong covalent bonds. There are also weak Van der Waals forces between the layers in Graphite.

66
Q

Explain why Iodine vaporises when heated gently.

A

The weak Van der Waals require little energy to break the forces between the molecules.

67
Q

State why Iodine is a very poor conductor of electricity.

A

The electrons are not delocalised therefore they are not free to move/carry the charge.

68
Q

Suggest a value for the bond angle in the H3O+ ion.

A

Angle: 107.

69
Q

Explain why the AsCl4(+) ion has a bond angle of 109.5.

A

AsCl4(+) has 4 bonded pairs of electrons. They repel equally, giving a bond angle of 109.5. The shape of the molecule is Tetrahedral.

70
Q

Shape of NHF2?

A

Trigonal Pyramidal.

71
Q

State the strongest type of Intermolecular force in Methane (CH4).

A

Van der Waals.

72
Q

State the strongest type of Intermolecular force in Ammonia (NH3).

A

Hydrogen Bonding.

73
Q

Suggest why Titanium can be hammered into different shapes.

A

Layers of atoms slide over one another.

74
Q

Deduce the empirical formula of Graphane.

A

CH.

75
Q

Why does Iodine sublime?

A

The weak Van der Waals forces between the molecules are easily overcome.

76
Q

Why do Simple Covalent Compounds have LOW boiling and melting points?

A

The covalent bonds within the molecules are strong but the forces of attraction between the molecules are weak (VdW).

77
Q

Simple Covalent Compounds are insoluble in water but soluble in…

A

Organic substances.

78
Q

The element with the larger electronegativity in a polar compound will be the…

A

Delta minus end.

79
Q

Why is Hydrogen Chloride a polar bond?

A

Chlorine is more electronegative than Hydrogen so it withdraws electron density from the covalent bond. The molecule has a dipole, a pair of separated charges of opposite signs.

80
Q

Why is CO2 non polar?

A

The two dipoles cancel each other out because they act in opposite directions. There is no net dipole.

81
Q

Explain why Boron Trifluoride molecules are non - polar but Water molecules are polar.

A

Boron Trifluoride has three dipoles that cancel each other out to leave no net dipole. The three atoms in water do not lie in a straight line, so it’s two dipoles do not cancel each other out leaving a net dipole.

82
Q

Are polar molecules usually symmetrical or asymmetrical?

A

Asymmetrical. Eg: Bent Planar / Trigonal Pyramidal

Chemistry : Unit 1 (6 decks)

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