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Chemistry > Topic 3: Structure And Bonding > Flashcards

Topic 3: Structure And Bonding Flashcards

1
Q

What are the properties of metals?

A
  • Dense.
  • Shiny.
  • Ductile- stretch into wires.
  • Good electric and thermal conductors.
  • They are all have regular arrangements.
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2
Q

Why are metals malleable and ductile?

A

-This is because they are made of a large 3D lattice, the layers can slip over each other.

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3
Q

What kind of structure does metallic bonding have?

A

-Giant Structure.

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4
Q

Different structures?

A
  • Face centered cubic E.g. Al.
  • Hexagonal close packed e.g. Mg.
  • Body centered cubic e.g. Na.
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5
Q

Define ionic bonding?

A

-Occurs between a metal and a non-metal- it is the complete transfer of one or more electrons metal to non-metal, giving charged ions that electrostatically attract.

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6
Q

Metals in groups 1,2,3?

A

-These can get full outer-shells most easily by losing all there outer electrons, to leave positive ions- this process is called oxidation.

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7
Q

Non-metals in groups 6-7?

A

-These can get to a full outer shell by accepting enough electrons from a metal to make hen up to a 8, forming negative ions- this process is called reduction.

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8
Q

Melting points of ionic compounds?

A

-This depends of the strength of the forces of attraction, this is therefore the melting point. The melting point increases as the charge increases. Eg Mg2+O2- has stronger forces of attraction then Na+Cl-.

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9
Q

What effects the charge density?

A
  • The size of an ion effects the strength of its forces of attraction.
  • Ten forces of attraction between two small ions will be greater then those between two large ions with the same charge.
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10
Q

Ionic bonding only occurs in?

A

-Giant structures.

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11
Q

Electrostatic forces ionic bonding?

A

-There are strong electrostatic forces between oppositely charged ions.

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12
Q

What are the properties of ionic sodium chloride NaCl?

A
  • High melting point.

- Non-conductive in its solid state, but when dissolved in water it becomes conductive.

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13
Q

Properties of ionic Magnesium oxide MgO?

A
  • Higher melting point then sodium chloride, because of more charge 2+ and 2- greater ionic bonds.
  • It also stays non-conductive because it stays solid at higher temperature.
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14
Q

Giant ionic substances form a…

A

-Giant ionic lattice.

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15
Q

Ionic solid properties?

A
  • High melting point.

- Don’t conduct when solid but they do when dissolved in solution.

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16
Q

How are ions formed?

A
  • Ions are electrically charged particles formed when atoms lose or gain electrons.
  • They have the same electronic structures as noble gasses.
  • Metal atoms lose electrons and form positive ions.
  • Non- metal gain electrons, atoms form negative ions.
  • The strong electrostatic forces of attraction between oppositely charged ions are called ionic bonds.
  • Ionic compounds have high melting and boiling points.
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17
Q

Examples of ionic bonds and ionic compounds?

A
  • NaBr sodium bromide.
  • KBr potassium bromide.
  • NaCl sodium chloride.
  • KI potassium iodide.
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18
Q

When do you get a covelent bond?

A

-When a non-metal and a non-metal need to bond.

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19
Q

What is a covalent bond?

A

-A bond with a shared pair of electrons. This is when two non-metals combine they both need to gain electrons, and they can do this by sharing two electrons in a covalent bond.

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20
Q

What is a simple molecular structure?

A

-This is a molecular structure that consists of small molecules, with weak forces of attraction (intermolecular forces between molecules).

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21
Q

Properties of Simple molecular?

A
  • They have low boiling points, so not much energy is needed to break the forces of attraction, also low melting points.
  • They do not conduct electricity at all as they have NO CHARGED PARTICLES.
  • Often dissolve in non-polar solvents such as hexane
  • Also insoluble in water.
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22
Q

Properties of Giant covalent structures?

A
  • They have many bonds 3-4.

- A lot of non-metal atoms each joined with covelent bonds.

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23
Q

Giant covelent lattice structure?

A

-Normally a giant arranged into giant regular latices- these are extremely strong because of the many bonds.

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24
Q

What is a Allotropes?

A

-When elements exist in more then one form such as carbon and diamond.

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25
Q

Properties of giant covalent?

A
  • They are hard.
  • They have very high melting points.
  • Insoluble in all solvents.
  • They don t conduct electricity in solid or when molten, this is because of the lack of charged particles.
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26
Q

Example of giant covelent?

A
  • Diamond- each atom is bonded to four neighbors, it is a crystal and very strong.
  • Graphite - honeycomb structure that has layers with strong covelent bonds holding them together.
  • It requires a lot of energy to break the strong covalent bonds.
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27
Q

Which to sub atomic particles make up the nucleus?

A

-Protons and neutrons.

28
Q

What is the mass of an electron?

A

-1/1860 know this

29
Q

What is the mass number?

A

-Amount of protons and neutrons.

30
Q

How to find the number of neutrons?

A

-Mass number - protons.

31
Q

What is the name given to the same element with a different number of neutrons?

A

-Isotope.

32
Q

Methane has a………boiling point. This is because it has…….. forces between the ………….

A
  • low
  • weak
  • molecules
33
Q

Why is hydrogen a gas at room temperature?

A

-This is because there is little energy need to overcome the forces of attraction.

34
Q

Why does magnesium chloride have a high melting point?

A

-Because the forces of attraction between the three ions is very strong, so it takes a lot of energy in the form of heat to pull them apart.

35
Q

Why does magnesium conduct electricity?

A

-Because it has many delocalized electrons which can carry a charge they are also free to move.

36
Q

Why does water have a low melting point?

A

-It has covelent bonds, it only has intermollecular forces holding it together, which are weak so it does not take a lot of energy to be overcome.

37
Q

Liquid sodium chloride conducts electric because..

A

-The charged ions are free to move.

38
Q

Diamond has a high melting point because…

A

-It has strong forces of attraction and also because it has four bonds to each atom.

39
Q

Magnesium can be stretched to form magnesium ribbon because….

A

-Atoms slide past each other, electrons prevent repulsion, it is also very malleable.

40
Q

Diamond is very hard because….

A

-It is in a 3D lattice structure, this is very strong and it takes a lot of energy to be pulled apart.

41
Q

What is the mass and charge of a proton?

A

-1amu positive.

42
Q

What is the mass and charge of a neutron?

A

-1amu no charge.

43
Q

The group number on the periodic table is also the same as…

A

-The number of outer electrons e.g. carbon group IV 4 outer electrons.

44
Q

What is a isotope?

A

-An isotope are elements whose atoms contain the same number of protons + electrons, but a different number of neutrons.

45
Q

Group number =

A

-The number of outer electrons.

46
Q

The Period number =

A

-The number of occupied electron shells.

47
Q

What are ions?

A

-Ions are charged particles that are formed when a neutral atom either gains or loses electrons. Atoms that lose electrons become positively charged (cations) and those that gain electrons become negatively charged (anions)

48
Q

If an atom gains electrons…

A

-It becomes negatively charged.

49
Q

If an atom loses electrons…

A

-It becomes positively charged.

50
Q

Metals lose electrons to form…

A

-Positive cations.

51
Q

Non-metals gain electrons to form…

A

-Negative anions.

52
Q

How is the periodic table organised?

A

-It is an arrangement of elements in order of atomic number

53
Q

What is a giant metallic structure?

A
  • Free electrons allow metals to conduct electricity and heat.
  • As the metals are made up of layers in a lattice, the layers can slip over each other, allowing the metal to be malleable and ductile.
54
Q

What are the noble gasses?

A

-The elements in group 0 are called the noble gases. They belong to the right-hand column in the periodic table. The noble gases are all chemically nonreactive which means they are inert.

55
Q

What properties do the noble gasses have in common?

A

-They are non-metals.
-They are very unreactive gases.
-They are colorless.
Tthey exist as single atoms (they are monatomic).

56
Q

Why are the noble gases so unreactive?

A

-All noble gases have the maximum number of electrons possible in their outer shell (2 for Helium, 8 for all others), making them stable.

57
Q

Why do elements in the same group of the periodic table have similar chemical properties?

A

-Elements in the same group in the periodic table have similar chemical properties. This is because their atoms have the same number of electrons in the highest occupied energy level. Group 1 elements are reactive metals called the alkali metals. Group 0 elements are unreactive non-metals called the noble gases.

58
Q

Oxidation is….

A

-The loss of electrons.

59
Q

Reductions is…

A

-The gain of electrons.

60
Q

What is ionic bonding?

A

-Ionic bonding is strong electrostatic forces of attraction between oppositely charged ions.

61
Q

How to calculate the relative abundance?

A

-Abundance 1 x mass 1 x abundance 2 x mass 2/ 100

62
Q

The periodic table is….

A

-The arrangement of elements in term of there atomic number.

63
Q

Why do group 0 have a lack of reactivity?

A

-This is because they have a full outer shell of electrons.

64
Q

Electronic configuration?

A

example, 2.8.5

65
Q

Example of an ionic formula?

A

Mg2+

66
Q

Describe the changes in the electronic configuration of sodium and chlorine when these atoms from sodium chloride. (3)

A

Sodium loses electrons.
Chlorine gains electrons.
Becoming 2,8 and 2,8,8

67
Q

The diatomic elements?

A 
- Bromine (Br) 
• Chlorine (Cl) 
• Fluorine (F) 
• Hydrogen (H) 
• Iodine (I) 
• Nitrogen (N) 
• Oxygen (O)

Chemistry (20 decks)

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