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Chemistry > Periodic Table > Flashcards

Periodic Table Flashcards

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1
Q

What are Groups in the Periodic Table?

A

Columns

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2
Q

What can the Group tell you about the Electrons in an Atom?

A

How many Electrons are in the Outer Shell

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3
Q

What are the Periods in the Periodic Table?

A

Rows

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4
Q

Why did Mendeleev put some Elements in Groups?

A

Similar Properties

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5
Q

Why did Mendeleev leave gaps in his Periodic Table?

A

Undiscovered Elements

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6
Q

What charge will an Ion of Lithium take?

A

1+

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7
Q

What charge will an Ion of Beryllium take?

A

2+

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8
Q

What charge will an Ion of Fluorine take?

A

1-

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9
Q

If something has gained Electrons, what charge will it have?

A

Negative

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10
Q

If something has lost Electrons, what charge will it have?

A

Positive

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11
Q

What charge will an Ion of Oxygen take?

A

2-

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12
Q

What charge will an Ion of Selenium take?

A

2-

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13
Q

What do Group 1 elements have in common?

A

1 Electron in Outer Shell

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14
Q

What do Group 7 elements have in common?

A

7 Electrons in Outer Shell

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15
Q

What do group 0/8 elements have in common?

A

Full Outer Shell

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16
Q

What’s more reactive, Lithium or Sodium?

A

Sodium

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17
Q

What’s more reactive, Chlorine or Bromine?

A

Chlorine

18
Q

Inert

A

Unreactive

19
Q

Why are Nobel Gases Inert?

A

Full Outer Shells

20
Q

What is a Trend?

A

A Pattern in Properties

21
Q

What is the Trend in the mpt’s of Alkali Metals?

A

Gets lower down the Group

22
Q

What state is fluorine at room temperature?

A

Gas

23
Q

What state is Chlorine at room temperature?

A

Gas

24
Q

What state is Bromine at room temperature?

A

Liquid

25
Q

What state is Iodine at room temperature?

A

Solid

26
Q

Balance: Li+ H2O= LiOH+ H2

A

2Li+ 2H2= 2LiOH+ H2

27
Q

Balance: K+ H2O= KOH+ H2

A

2K+ 2H2O= 2KOH+ H2

28
Q

LiOH

A

Lithium Hydroxide

29
Q

KOH

A

Potassium Hydroxide

30
Q

Why are Group 1 elements called Alkali Metals?

A

They are Metals that form Alkalis when they react with Water

31
Q

What is a Displacement Reaction?

A

A more reactive Element takes the place of a less reactive Element in a Compound

32
Q

Why doesn’t KBr+ I2 react?

A

Iodine is less reactive than Bromine so won’t displace it

33
Q

Balance KBr+ Cl2= KCl+Br2. Why is it a displacement reaction?

A

2KBr+ Cl2= 2KCl+ Br2

Chlorine has displaced Bromine as its more reactive

34
Q

Why is Fluorine more reactive than Chlorine?

A

Fewer shells, less shielding, easier to gain Electrons

35
Q

Why is Potassium more reactive than Lithium?

A

More shells, less shielding, easier to lose Electrons

36
Q

Why is Bromine less reactive than Chlorine?

A

More shells, more shielding, harder to gain electrons

37
Q

Why is Sodium less reactive than Caesium?

A

Fewer shells, less shielding, harder to lose electrons

38
Q

Where are Transition Metals found in the Periodic Table?

A

In the Middle

39
Q

Compare mpt, density, strength, hardness and reactivity of Transition metals with Group 1 Metals

A

Higher for all but Reactivity

40
Q

What is distinctive about the Ions formed by Transition Metals?

A

Can form Ions with different charges

41
Q

What is distinctive about the Compounds formed from Transition Metals?

A

They are Coloured

42
Q

What can Transition Metals be used for?

A

Catalysts

Chemistry (4 decks)

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