chapter 14: the periodic table Flashcards

1
Q

how are the elements of the periodic table arranged

A

in increasing proton number

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2
Q

What are horizontal rows of elements in the periodic table called?

A

periods

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3
Q

what are vertical columns of elements in the periodic table called?

A

groups

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4
Q

What are elements close to the ‘zig-zag’ line called?

A

metalloids

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5
Q

name the metalloids
(7 of them)

A

boron
silicon
germanium
arsenic
antimony
tellurium
polonium

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6
Q

what are the properties of metals

A
  • high melting and boiling points
  • shiny
  • ductile, malleable
  • sonorous
  • good conductors of heat and electricity
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7
Q

what are the properties of metalloids

A

it has properties of metals and non-metals

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8
Q

what are the properties of non-metals

A
  • gaseous or volatile
    liquid or dull, brittle solids
  • low melting points
  • poor conductors of heat and electricity
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9
Q

why is there an increase in metallic character with increasing atomic size?

A

as the valence electrons are further away from the nucleus, the elements have a greater tendency to lose the valence electron to form positive ions

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10
Q

period number = number of _______ _______

A

electron shells

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11
Q

group number = number of ________ _________

A

valence electrons

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12
Q

elements on the same group have similar ______________

A

chemical properties

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13
Q

physical properties of group 1 metals
(alkali metals)
I

A
  • shiny and soft
  • very good conductor of heat and electricity
  • low melting and boiling points (decreases down the group)
  • low density (decreases down the group)
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14
Q

chemical properties of group 1 metals

A
  • alkali metals are highly reactive. to prevent them from reacting with air or water, they are stored under oil.
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14
Q

why are group 1 metals very chemically reactive?

A

they are all very chemically reactive as they all just have one electron in their outermost shell and therefore form M+ ions (Li+, Na+, K+). As we go down group 1, the reactivity of the alkali metals increases as it becomes easier to lose their outermost electron.

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15
Q

physical properties of group 7 elements
(halogens)
VII

A
  • coloured (becomes darker down the group)
  • low melting and boiling points (increases down the group)
16
Q

Flourine
- appearance
- melting point
- boiling point
- state at r.t.p.

A
  • pale yellow
  • melting: -220
  • boiling: -188
  • rtp state: gas
17
Q

Chlorine
- appearance
- melting point
- boiling point
- state at r.t.p.

A
  • greenish-yellow
  • melting: -101
  • boiling: -34
  • rtp state: gas
18
Q

Bromine
- appearance
- melting point
- boiling point
- state at r.t.p.

A
  • reddish-brown
  • melting: -7
  • boiling: 59
  • rtp state: liquid
19
Q

Iodine
- appearance
- melting point
- boiling point
- state at r.t.p.

A
  • shiny-black / purplish black
  • melting: 114
  • boiling: 184
  • rtp state: solid
20
Q

Lithium reaction with water

A

reacts quickly. the metal floats on the surface of water
no flame observed

2Li (s) + 2H2O (l) –> 2LiOH (aq) + H2 (g)

21
Q

Alkali metals react vigorously with water to form ………

A

the alkaline hydroxide and liberating hydrogen gas

22
Q

Sodium reaction with water

A

reacts violently. the metal darts around the water surface. reaction may be explosive.
hydrogen gas catches fire and burns with a yellow fire.

2Na (s) + 2H2O (l) –> 2NaOH (aq) + H2 (g)

23
Q

Potassium reaction with water

A

reacts very violently. the metal darts about the water surface. reaction is explosive.
hydrogen gas catches fire and burns with a lilac flame

2K (s) + 2H2O (l) –> 2KOH (aq) + H2 (g)

24
Q

Because alkali metals are so reactive, they will combine directly with other non-metals, such as ……..

A

halogens

25
Q

Sodium burns in chlorine gas to produce…..

A

a white smoke of sodium chloride (common salt)

2Na (s) + Cl2 (g) –> 2NaCl (s)

26
Q

why are alkali metals powerful reducing agents?

A

alkali metals lose their valence electron easily to obtain the stable noble gas electronic configuration

27
Q

Astatine
- appearance
- melting point
- boiling point
- state at r.t.p.

A
  • black
  • melting: 302
  • boiling: 337
  • rtp state: solid
28
Q

group 7 (VII) elements exist as……..
clue: F2, Cl2, Br2, I2

A

covalent, diatomic molecules

29
Q

to attain a stable octet configuration, group 7 elements need to…..

A

attract one more electron

30
Q

halogens react with most metals to form….

A

metal halides

31
Q

examples of metal halides

A

NaCl
KCl
MgCl2
ZnCl2

32
Q

group 0 elements are also known as

A

inert or noble gases

33
Q

physical properties of group 0 elements

A
  • colourless
  • odourless
  • gaseous state at rtp
  • low melting and boiling points
  • insoluble in water
34
Q

chemical properties of group 0 elements

A
  • chemically inert (unreactive)
    they have a completely filled valence shell, they do not gain, lose, or share electrons to form compounds
  • monatomic
    (consisting of one atom)