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Chemistry _Amma > Bonding > Flashcards

Bonding Flashcards

1
Q

What are the two broad types of elements?

A

Metals and non-metals

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2
Q

How does the position of metals on the Periodic Table affect their outer shell electrons?

A

Metals further to the left have fewer electrons in their outer shells.

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3
Q

How are elements arranged on the periodic table?

A

Increasing atomic number

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4
Q

What is the maximum number of electrons that can be held in the second shell?

A

8

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5
Q

What group is chlorine in on the Periodic Table?

A

7

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6
Q

What are elements that display properties of both metals and non-metals called?

A

Metalloids or semi-metals

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7
Q

What happens to the outer shell electrons as you descend a group on the Periodic Table?

A

They become further from the nucleus due to increasing atomic size.

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8
Q

What do vertical columns on the periodic table represent?

A

Groups

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9
Q

Why do atoms react with other atoms?

A

To achieve a full outer shell of electrons

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10
Q

What trend occurs due to atoms more readily accepting electrons to fill their valence shells?

A

Electron affinity

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11
Q

How does the position of a metallic element in a group affect its reactivity?

A

The further down the group, the easier it reacts by losing outer electrons.

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12
Q

What do horizontal rows on the periodic table represent?

A

Periods

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13
Q

What is important to remember when drawing electronic structures?

A

All shells up to the outer shell will be full

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14
Q

What are positive ions called?

A

Cations

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15
Q

How is the reactivity of non-metallic elements affected by their position in a group?

A

The further down the group, the harder it is to gain electrons and react.

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16
Q

How many electron shells do elements in Period 2 have?

A

Two

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17
Q

What is another name for energy level?

A

Shell

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18
Q

What are negative ions called?

A

Anions

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19
Q

What is the characteristic of Group 1 elements?

A

One outer shell electron

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20
Q

How many electron shells do elements in Period 3 have?

A

Three

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21
Q

What does the number of numbers in an electronic configuration indicate?

A

Number of shells

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22
Q

What is the characteristic of Group 2 elements?

A

Two outer shell electrons

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23
Q

What do the vertical columns in the periodic table represent?

A

The number of outer electrons

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24
Q

What do elements in the same group have in common?

A

Same number of outer shell electrons

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25
Q

What is an ion?

A

Charged atom or molecule

26
Q

What is the characteristic of Group 0 (Group 8) elements?

A

Full outer shells

27
Q

What is Group 1 known as?

A

Alkali metals

28
Q

What happens to an atom when it ends up with fewer electrons?

A

Positive ion

29
Q

What is Group 7 known as?

A

Halogens

30
Q

What type of ions do non-metals form when they react?

A

Negative ions

31
Q

Why does the attraction between outer shell electrons and the nucleus weaken as you descend a group?

A

Because the outer shell electrons are further away from the nucleus.

32
Q

What is Group 0 known as?

A

Noble gases

33
Q

How does metallic character change across a Period on the Periodic Table?

A

Decreases from left to right

34
Q

What key difference affects the chemical behaviour of metals and non-metals?

A

Metals easily lose electrons, non-metals find it difficult to gain electrons.

35
Q

What is the outermost shell of an atom called?

A

Valence shell

36
Q

How do non-metals form anions?

A

Gain electrons

37
Q

How do metals form cations?

A

Lose electrons

38
Q

How many shells of electrons does a chlorine atom have?

A

3

39
Q

How does metallic character change down a Group on the Periodic Table?

A

Increases

40
Q

What does an element’s position on the Periodic Table indicate about its reactivity?

A

It shows a link between atomic number and how easily it can lose or gain electrons.

41
Q

What is the significance of each element having one proton more than the element preceding it?

A

Starts with one electron more

42
Q

How can atoms form covalent bonds?

A

Share electrons

43
Q

What do you need to remember the terms for in many chemistry topics?

A

Positive and negative ions

44
Q

How are periods numbered on the periodic table?

A

01-Jul

45
Q

How should you spread out 1, 2, 3, or 4 electrons in a shell?

A

One per quarter of the shell

46
Q

Can you share a mnemonic for remembering positive ions?

A

‘CATions are PAWsitive’

47
Q

How are the groups in the periodic table numbered?

A

From 1 to 7, with a final group 0

48
Q

How should you distribute 5, 6, 7, or 8 electrons in a shell?

A

In pairs or equally spread out

49
Q

Can you share a mnemonic for remembering negative ions?

A

‘ANions are A Negative ion’

50
Q

How can we represent the electronic structure of atoms?

A

Electron shell diagrams

51
Q

What should you make sure of when using dots or crosses to represent electrons in a shell?

A

On the line of that shell

52
Q

Where do electrons orbit in atoms?

A

Shells

53
Q

What does the number of outer shell electrons indicate?

A

Group number

54
Q

Why do metals form positive ions when they react?

A

They lose electrons

55
Q

What does the number of shells of electrons indicate?

A

Period

56
Q

What are the characteristic properties of metals and non-metals?

A

A summary of general properties

57
Q

What is another name for Group 0 in the periodic table?

A

Group 8

58
Q

How many outer electrons does chlorine have?

A

7

59
Q

Do all electron shells have the same energy associated with them?

A

No

60
Q

Why is an atom much more stable if it can completely fill its valence shell with electrons?

A

Stability

Chemistry _Amma (8 decks)

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