The periodic Table (3) βœ… Flashcards

1
Q

Who + when developed the modern periodic table

A

Dmitri Mendeleev, 1869

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2
Q

What are the 5 main properties of Dmitri Mendeleev’s periodic table

A
  • arranged in order of increasing atomic mass
  • Left gaps for undiscovered elements
  • No noble gases
  • No transition metal block
  • No actinides or lanthanides
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3
Q

What are the 5 main properties of the modern periodic table

A
  • arranged in order of increasing atomic number
  • no gaps left
  • Noble gases present
  • Block of transition metals between group 2+3
  • actinides and lanthanides present
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4
Q

what are the group 1 elements called?

A

The alkali metals - the most reactive metals

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5
Q

what are the group 7 elements called?

A

The halogens - the most reactive non-metals

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6
Q

what are the group 0 elements called?

A

The noble gases - unreactive non metals

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7
Q

what are the group 2 elements called?

A

Alkaline earth metals - less reactive than group 1

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8
Q

what is the block of elements between group 2+3 called?

A

the transition metals - form coloured compounds and their unreactive metals

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9
Q

what is the most reactive metal

A

francium

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10
Q

what is the most reactive non metal

A

fluorine

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11
Q

what are the two semi metals

A

Silicon, germanium

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12
Q

what are the vertical columns on the periodic table called

A

groups

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13
Q

what are the horizontal rows on the periodic table called

A

periods

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14
Q

floats, moves, bubbles, heat, disappears ,solution, universal indicator

what observations are observed when Lithium (Li) reacts with water

A

metal floats, moves on surface, bubbles of gas, heat released, Li disappears, colourless solution forms, universal indicator turns purple

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15
Q

what is the equation for Lithium reacting with water

A

2Li + 2H2O –> 2LiOH + H2

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16
Q

what observations are observed when Sodium (Na) reacts with water

A

metal floats, moves on surface, bubbles of gas, heat released, Na melts and forms ball, Na disappears, colourless solution forms, universal indicator turns purple

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17
Q

what is the equation for sodium reacting with water

A

2Na + 2H2O β€”> 2NAOH + H2

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18
Q

what observations are observed when Potassium (K) reacts with water

A

metal floats, moves on surface, burns with lilac flame, heat released, bubbles of gas, K disappears, colourless solution forms, universal indicator turns purple

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19
Q

what is the equation for potassium reacting with water

A

2K + 2H20 –> 2KOH + H2

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20
Q

Name 5 safety precautions we always take when using alkali metals

A
  • safety screen
  • hair up and goggles worn
  • metal handled with tweezers
  • small pieces used
  • large volume of water
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21
Q

how are alkali metals stored and why?

A

under oil - to prevent reaction with oxygen and moisture in the air

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22
Q

how many electrons do alkali metals have in their outer shell
(group 1)

A

1

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23
Q

when alkali metals react they lose how many electrons?

and form what type of bond with non-metals

A

one

ionic bonds

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24
Q

name 3 characteristics of alkali metals

A

soft, shiny, tarnish quickly

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25
Q

What do alkali metals form when they react?

A

A positive ion (cation)

Alkali metals lose one electron during the reaction.

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26
Q

Why do alkali metals have similar chemical properties?

A

They react by losing one electron to form stable cations

This results in a full outer shell of electrons.

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27
Q

What charge do the cations formed by alkali metals carry?

A

A single positive charge

This charge reflects the loss of one electron.

28
Q

Fill in the blank: Alkali metals lose one electron to form a _______.

A

positive ion (cation)

This process leads to stability in the ion.

29
Q

What characteristic of cations contributes to their stability?

A

A full outer shell of electrons

This is a common trait in stable ions.

30
Q

What is the color of most group 1 compounds?

31
Q

Do most group 1 compounds dissolve in water?

32
Q

What type of solutions do most group 1 compounds give when dissolved in water?

A

Colourless solutions

33
Q

What are group 7 elements known as?

A

Halogens

Halogens are reactive non-metals.

34
Q

How many electrons do halogens have in their outer shell?

A

7 electrons

This electron configuration contributes to their reactivity.

35
Q

What is the valency of halogens?

A

1

This means they need one electron to achieve stability.

36
Q

What do halogens need to be stable?

A

One electron

Acquiring one electron allows them to achieve a full outer shell.

37
Q

In what form do halogens exist when unreacted?

A

Diatomic molecules

Examples include Cl2, Br2, I2.

38
Q

What is an example of a diatomic molecule formed by a halogen?

A

Cl2

Other examples include Br2 and I2.

39
Q

What happens to iodine when heated?

A

The grey-black solid changes to a purple vapour.

40
Q

What is the process called when a solid changes directly to a gas?

A

Sublimation.

41
Q

What occurs when iodine cools after being heated?

A

It changes back to grey-black crystals.

42
Q

True or False: Sublimation is the process of a solid turning into a liquid.

43
Q

Fill in the blank: The grey-black solid iodine changes to a _______ vapour when heated.

44
Q

what does aquinas mean

A

mixed with water

45
Q

what happens when iodine or bromine (halogens) is mixed with sodium chloride solution

A

no reaction

46
Q

what happens when sodium bromide solution is mixed with chlorine

A

colourless solution turns orange

47
Q

what happens when sodium bromide solution is mixed with iodine

A

no reaction

48
Q

what happens when sodium iodide solution is mixed with chlorine or bromine

A

colourless solution turns brown

49
Q

reacitivity

What trend in reactivity is observed in group 7 halogens?

A

Reactivity decreases going down group 7.

50
Q

What does a more reactive halogen do to a less reactive halogen in an aqueous solution?

A

A more reactive halogen will displace a less reactive halogen from its salt solution.

51
Q

Why do halogens have similar chemical properties?

A

Because when they react, an atom gains one electron to form a negative ion (anion) with a full outer shell of electrons.

52
Q

What charge does a stable halogen ion have?

A

A single negative charge.

53
Q

Fill in the blank: The ion formed by halogens after gaining an electron is called a _______.

A

negative ion (anion).

54
Q

True or False: All halogens react by losing an electron.

55
Q

What happens to the electron configuration of a halogen atom when it reacts?

A

It gains one electron to achieve a full outer shell.

56
Q

What happens to the number of electron shells as you move down Group 7?

A

The atoms have more shells of electrons

57
Q

How does the distance of the outermost shell from the nucleus change down Group 7?

A

The outermost shell is further from the positive attraction of the nucleus

58
Q

What effect does the increased distance from the nucleus have on the attraction of incoming electrons?

A

The force of attraction decreases

59
Q

What is the trend in reactivity as you move down Group 7?

A

Reactivity decreases

60
Q

True or False: The reactivity of elements in Group 7 increases as you go down the group.

61
Q

What is the test for chlorine?

A

universal indicator paper turns red then bleaches white

62
Q

What are Group 0 elements known as?

A

Noble gases

Group 0 elements are characterized by their lack of reactivity due to having a complete valence shell.

63
Q

What is a defining characteristic of noble gases?

A

Unreactive non-metals

Noble gases do not easily form chemical compounds with other elements.

64
Q

physical properties of transition metals

A

high melting point (except mercury)
high density
low reactivity - some react with steam

65
Q

physical properties of Group 1 metals

A

low melting point
Low density
very reactive with water