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Chemistry > Structure and bonding > Flashcards

Structure and bonding Flashcards

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0
Q

What are atoms?

A

What elements are made from. An atom consists of a nucleus containing protons and neutrons surrounded by electrons.

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1
Q

What are ions?

A

Ions are electrically charged particles formed when atoms lose or gain electrons. They have the same electronic structures as noble gases.

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2
Q

What’s an electron?

A

An electron is a very small negatively charged particle found in an atom in the space surrounding the nucleus.

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3
Q

What form positive ions and what form negative ions?

A

Metal atoms form positive and non metal atoms form negative ions.

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4
Q

What are ionic bonds?

A

The strong electrostatic forces of attraction between oppositely charges ions.

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5
Q

Ionic compounds have _____ melting and boiling points.

A

High

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6
Q

What’s an ionic compound?

A

An ionic compound occurs when a negative ion joins with a positive ion. The ions swap electrons to achieve a full outer shell.

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7
Q

What’s a negative ion?

A

An atom that has gained an electron.

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8
Q

What’s a positive ion?

A

An atom that has lost an electron.

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9
Q

What do metal atoms do?

A

They lose the electron in their highest energy level and become positively charged ions.

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10
Q

What do non metals atoms do?

A

They gain an electron from another atom to become negatively charged ions.

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11
Q

What’s a covalent bond?

A

A covalent bond between atoms forms when atoms share electrons to achieve a full outer shell of electrons. This is between atoms of non metallic.

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12
Q

Fill gaps:
When metals react with non-metals, _________are transferred from the metal atoms to the non metals atoms, forming ______.
This resulting an _______ __________.

A

Electrons
Ions
Ionic compound

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13
Q

Why does it take a great deal of energy to separate the positive and negative ions in a crystal lattice?

A

Because of the strong electrostatic forces between them.

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14
Q

Why don’t solid ionic compounds conduct electricity?

A

Because the ions are held firmly in place they cannot move to conduct the electric current.

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15
Q

What happens to an ionic compound when it melts?

A

The charged ions are free to move

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16
Q

What happens when a crystal of an ionic compound dissolves in water?

A

The ions separate, and again the ions are free to move ,so a solution of an ionic compound in water also conducts electricity.

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17
Q

Why do ionic bonds have high melting and boiling points?

A

Ionic bonds are very strong so a lot of energy is needed to break them.

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18
Q

How can you tell that the compound h2o has covalent bonds?

A

It’s made up of non metals.

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19
Q

Explain what happens to the atoms of the elements when lithium reacts with fluorine.

A

Lithium atoms lose an electron to form a lithium that has a positive charge. Fluorine atoms gain an electron to form a fluorine that has a negative charge.

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20
Q

Metal atoms______ electrons to become stable forming ______ ions.

A

Lose

Positive

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21
Q

Non metal atoms ______ electrons to become stable forming ________ ions.

A

Gain

Negative

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22
Q

Group one charge

A

+1

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23
Q

Group two charge

A

+2

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24
Q

Group three charge

A

+3

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25
Q

Group five charge

A

-3

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26
Q

Group six charge

A

-2

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27
Q

Group seven charge

A

-1

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28
Q

What is formed when two or more elements react together?

A

Compounds

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29
Q

To achieve stable electronic structures what do the atoms of elements do?

A

They join together by sharing electrons or by transferring electrons to achieve stable electronic structures.

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30
Q

What group have stable electronic structures?

A

Noble gases

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31
Q

Fill in the gaps:

When atoms of non-metallic elements join together by sharing electrons it is called ________ __________.

A

Covalent bonding

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32
Q

How can you tell that the compound H2O has covalent bonds?

A

It is made up of non metals

33
Q

What’s the name of the compound produced when a metallic element reacts with a non metallic element?

A

Ionic compounds

34
Q

In ionic compounds what happens to the metal atoms?

A

They lose electrons to form positive ions

35
Q

In ionic compounds what happens to the non metal atoms?

A

They gain electrons to form negative ions

36
Q

Fill in the gaps:

The ions have the _________ electronic structure of a noble gas.

A

Stable

37
Q

Fill in the gaps:

The oppositely charged ions attract each other in the ionic compound and this is called _________ ____________.

A

Ionic bonding

38
Q

Which of these compounds have ionic bonding?

KBr, HCl, H2S, Na2O, Cl2O, MgO

A

KBr, Na2O, MgO

39
Q

How many electrons are in the atoms of elements in group 1?

A

One electron in outer shell

40
Q

What is the electronic structure of sodium?

A

2.8.1

41
Q

Give the ion and electronic structure of sodium

A

Na+ , 2.8

42
Q

How many electrons are on the outer shell of group 7 elements?

A

7 electrons on outer shell

43
Q

Give the ion and new electronic structure of chlorine

A

Cl-

2.8.8

44
Q

Give the formula of sodium chloride

A

NaCl

45
Q

Explain what happens to the atoms of the elements when lithium reacts with fluorine.

A

Lithium atoms lose an electron to form a lithium ion that has a positive charge or Li+ , fluorine atoms gain an electron to form a fluorine ion that has a negative charge or F-

46
Q

How are ionic compounds held together?

A

By strong forces between the oppositely charged ions. This is called ionic bonding.

47
Q

Fill in the missing gap:

Ionic bonding holds oppositely charged ions together in _________ __________.

A

Giant structures

48
Q

Why is the giant structure of ionic compounds very regular?

A

Because the ions all pack together neatly like marbles in a box.

49
Q

Where do strong electrostatic forces of attraction act in?

A

In all directions

50
Q

What is each ion in the giant structure or lattice surrounded by?

A

By ions with opposite charge and so is held firmly in place.

51
Q

What does the ratio of ions in the structure of an ionic compound depend on?

A

On the charge on the ions.

52
Q

How can we represent ions and atoms?

A

Using/drawing a dot and cross diagram.

53
Q

Why is the formula of sodium chloride NaCl but magnesium chloride is MgCl2?

A

Sodium ions have a single positive charge (Na+) and magnesium ions have a double positive charge (Mg2+)
Chloride ions have a single negative charge.

54
Q

What are dot cross diagrams used for?

A

Used to represent the atoms and ions involved in forming ionic bonds.

55
Q

What shell do we show in dot cross diagrams?

A

The outer shell

56
Q

What do the charges on ions in an ionic compound do?

A

Always cancel each other out

57
Q

What does the formula of an ionic compound show?

A

It shows the ratio of ions present in the compound.

58
Q

What’s the relative charge for proton, neutron and electron?

A

Proton: +1
Neutron: 0
Electron: -1

59
Q

What’s the formula of an chlorine ion?

A

Cl-

60
Q

What’s the formula of a magnesium ion?

A

Mg2+

61
Q

What’s the formula of the ion phosphorus?

A

P3+

62
Q

What’s the electronic structure of the ion chlorine?

A

(2.8.8)-

63
Q

What’s the electronic structure of the ion magnesium?

A

(2.8)2+

64
Q

What’s the electronic structure of the ion phosphorus?

A

(2.8.8)3-

65
Q

Fill in the gaps:
When sodium reacts with chlorine, sodium ________ an electron and chlorine _________ an electron. When sodium atoms become sodium ions this is called __________. When chlorine atoms become __________ ions this is called _________.

A 
Loses
Gains
Oxidation 
Chloride
Reduction
66
Q

Why do ionic compounds have high melting points?

A

There’s strong ionic bonds between the ions so they require a large amount of energy to break.

67
Q

Describe under what circumstances ionic substances do and do not conduct electricity?

A

Do- when the substances dissolved in water and when the substance is melted/molten this is because the ions have more space to move.
Don’t - when they are solid because the ions aren’t free to move around.

68
Q

Why are ionic substances brittle?

A

The forces align with the same charge, and the ions repel and as a result break.

69
Q

Would you expect calcium oxide to have a higher or lower melting point than potassium fluoride?

A

Yes, I would expect the calcium oxide to have a higher melting point than KF , because the charges are double positive and double negative, this will mean that the electrostatic forces between Ca and O will be much stronger than K and Br.

70
Q

How are calcium and chlorine combined what type of compound?

A

Ionic bonding because calcium is a metal and chlorine is a non metal.

71
Q

How are carbon and oxygen bonded- what bond?

A

Covalent, because carbon and oxygen are both non metals.

72
Q

When a metal and non metal transfer electrons forming ions what type of bonding is this called?

A

Ionic bonding

73
Q

How do two or more non metals share electrons?

A

Covalent bonding

74
Q

Why do atoms bond?

A

To get stable electron arrangements.

75
Q

Fill in the gaps:

Metal atoms ________ electrons to become stable forming __________ ions.

A

Lose

Positive

76
Q

Fill in the gaps:

Non- Metal atoms ________ electrons to become stable forming __________ ions.

A

Gain

Negative

77
Q

Give the charge of groups 1,2,3,4,5,6,7,0

A 
Group1: +1
Group2: +2
Group3: +3
Group 4 don't usually form ions 
Group5: -3
Group6: -2
Group7: -1
78
Q

To cancel each other out, on the positive and negative ions what has to be the same?

A

The electrons lost must equal the electrons gained.

79
Q

What are the charges of carbonates?

A

CO32-

Chemistry (11 decks)

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