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Chemical Bonding Flashcards

1
Q

What are the three types of chemical bonding?

A
  • Ionic
  • Covalent
  • Metallic
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2
Q

When does ionic bonding occur?

A

Only found in compounds
Between the most reactive metals and non-metals

E.g. Potassium Chloride

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3
Q

When does covalent bonding occur?

A

Found amongst elements and compounds
Between non-metals

E.g. Water is a covalent bond

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4
Q

When does metallic bonding occur?

A

Found only in metals

E.g. Lithium

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5
Q

Why do atoms join together?

A

Atoms other than those of noble gases have incomplete outer shells and form chemical bonds in order to pair up all unpaired electrons, and so acquire the electronic structure of the nearest noble gas.

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6
Q

Why does ionic bonding happen?

A

Because the ions are oppositely charged they are attracted to each other, thus forming an electrostatic bond.

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7
Q

What is ionic bonding?

A

When two atoms both don’t have complete outer shell they transfer each other the extra electrons they need to have full outer shells.

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8
Q

What is it called once it has bonded ionicly?

A

Ion

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9
Q

What is an example of ionic bonding?

A

Lithium-2,1
Fluorine-2,7
Lithium has lost 1 electron so ends up have 2 on its outer shell and gets a charge of +1 written as Li^+
Fluorine has gained 1 electron so ends up with 8 on its outer shell and gets a charge of -1 written as F^-
The formula for this bond is LiF
*note-you can have multiple of one atom to bond to another

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10
Q

How do you draw diagrams for ionic bonding?

A

You draw the two atoms how they are then draw an arrow between them going down and below you draw them with full outer shells in big square brackets and outside the square brackets you put the charge also if you need 2 of one atom you draw a big 2 next to that atom.

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11
Q

Properties of Ionic compounds

A
  • crystalline
  • brittle
  • oppositely charged ions attract each other packing themselves into a lattice structure
  • high melting and boiling points because to allow the ions to move you need to overcome the electrostatic force of attraction between the ions, since the force the energy required to overcome it is large so the melting point is high
  • the higher the charges on the ions the stronger the attraction
  • solid at room temperature
  • many soluble in water but insoluble in organic solvents
  • don’t conduct electricity in solid state but do when the compound is molten or soluble in water(an aqueous solution) due to the ions being able to move when in a liquid
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12
Q

What happens when an atom loses/gains an electron?

A

Loses-becomes positively charged

Gains-become negatively charged

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13
Q

What relation is there between the periodic table group number and the overall charge of the ion?

A 
Group1-loses electron-charge 1+
Group2-loses electrons-charge 2+
Group3-loses electrons-charge 3+
Group5-gains electrons-charge 3-
Group6-gains electrons-charge 2-
Group7-gains electron-charge 1-
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14
Q

Hydroxide?

A

_

OH

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15
Q

Sulphate?

A

2-
SO
4

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16
Q

Carbonate?

A

2-
CO
3

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17
Q

Hydrogen carbonate?

A

_
HCO
3

18
Q

Nitrate?

A

_
NO
3

19
Q

Ammonium?

A

+
NH
4

20
Q

What are the charges for the transition metals?

A

(The elements between group 2 and 3)
The charge is given by a Roman numeral after its name
+ 2+
E.g. Copper(I) is Cu ; Copper(II) is Cu

21
Q

Zinc?

A

2+

Zn

22
Q

Silver?

A

+

Ag

23
Q

Hydrogen?

A

+

H

24
Q

Ionic formulae?

A

You have to get the two atoms to have an overall charge of 0

  • how ever many of one atom you need you put the number at the bottom(small number)
  • the ions which you have to learn put them in brackets and put the number outside
  • PUT THE POSITIVE ION BERORE THE NEGATIVE ION
  • DON’T INCLUDE THE CHARGE FOR FORMULAE
25
Q

How does Covalent bonding work?

A

Atoms share their electrons and pair up
They stay slightly overlapped because there is an attraction the two nuclei(an electrostatic attraction)
A shared pair of electrons is referred to as a single covalent bond

26
Q

What three ways can represent covalent bonding?

A

1) by drawing the outer shells as circles overlapping with dots and crosses on
2) just drawing dots and crosses between the two atoms(NO CIRCLES)
3) just draw lines between the two atoms

27
Q

Covalent bond can be defined as?

A

The electrostatic attraction between a pair of electrons and the nuclei of two atoms

28
Q

How do you represent multiple bonds?

A

If there are more than one electron being shared

1) you have to draw more than one between the overlapping shells
2) just draw more than one dot and cross between the two atom symbol
3) just draw more than one line between the two atoms

29
Q

Giant covalent structures?

A 
All from carbon
Also known as macro molecules
-diamond
-graphite
-fullerenes
30
Q

Properties of diamond?

A

Carbon

  • all 4 outer electrons Form covalent bonds
  • 3D structure formed
  • each carbon atoms forms 4 bonds to other carbon atoms
  • no weak intermolecular forces
  • very high melting point
  • very hard and abrasive
  • doesn’t conduct electricity
  • used for cutting tools and diamonds
31
Q

Properties of graphite?

A

Carbon

  • 3 outer electrons used to form covalent bonds(the fourth becomes a delocalised electron)
  • layered structure formed
  • weak intermolecular forces between the layers
  • high melting point
  • soft and slippery
  • conducts electricity(because of the delocalised electron)
  • used lubricant, pencils
32
Q

Properties of covalent substances?

A

Structure
-simple molecular-exist as small molecules
-macro molecular-exist as giant structures
Melting points
-simple molecular-low melting points(intermolecular forces are weak)
-macro molecular-high melting points(no intermolecular forces)
Conductivity
-simple molecular-don’t conduct electricity
-macro molecular-Graphite conducts electricity
Solubility
-simple molecular-insoluble in water but soluble in organic solvents
-macro molecular-insoluble

33
Q

What is metallic bonding?

A

When many of the same metal atom form a giant structure(lattice) since all extra electrons become delocalised electrons so for example lithium would become a lithium ion(Li^+) which is positively charged and thus attracted(strong electrostatic attraction) to the negatively charged ‘sea of electrons’(delocalised electrons)

34
Q

What are the properties of metals?

A

Conductivity
-conduct electricity and heat in a solid state
Melting point
-high(strong force between the delocalised electrons)
Malleability and ductility
-when a force is applied to a metal the layers can slide over each other
(Malleability able to be hammered into different shapes)
(Ductility able to be pulled into a wire)

35
Q

Sodium chloride is a solid with a high melting point?

A

There are strong electrostatic attraction between positive and negative ions which takes a lot of energy to break

36
Q

Copper metal conducts electricity?

A

Delocalised electrons can move(and carry current)

37
Q

Hydrogen is a gas?

A

Weak intermolecular forces between the molecules which are easily broken

38
Q

Diamond is a hard solid?

A

The carbon atoms are bonded by strong covalent bonds in a rigid 3D structure

39
Q

Graphite is relatively soft?

A

The carbon atoms are arranged in layers which have weak intermolecular forces between them and can slide over each other

40
Q

Why are metals malleable?

A

Because of the lattice/layered structure which forms from metallic bonding, the atoms can slide over each other so they can be bent and won’t break

41
Q

Why does diamond have a high melting point?

A
  • Giant covalent structure
  • held together by strong covalent bonds
  • to melt it you have to break a lot of strong covalent bonds
  • you need a lot of energy to break these bonds thus a high melting point
42
Q

Why does fullerene, a simple molecular structure have a low melting point?

A
  • You only have to overcome weak forces of attraction between the fullerene molecules(weak intermolecular forces)
  • don’t break bonds
  • takes less energy to break weak intermolecular forces than covalent bonds

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