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Chem > Chapter 13 Behavior of metals > Flashcards

Chapter 13 Behavior of metals Flashcards

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1
Q

what are group 1 metals called

A

alkali metals

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2
Q

how does reactivity change down the group and why (group 1)

A

reactivity increases

there is a lesser force of attraction between the outer shell electron and the nucleus, as the shell number increases the force of attraction will decrease making it easier to give the electron away.

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3
Q

how does the melting and boiling point change down the group and why (group 1)

A

melting and boiling point decrease down the group

as the reactivity increases, it is easier to break the bonds hence making it easier to melt or boil

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3
Q

how does the softness change down the group and why (group 1)

A

softness increases

as the reactivity increases, the bonds become easier to break, making the metal softer and easier to cut

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4
Q

how does the density change down the group and why (group 1)

A

density increases

as the mass number increases there will be more particles per unit volume increasing the density

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5
Q

what are group 2 metals called

A

alkaline earth metals

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6
Q

what are the trends as you go down the group (group 2 metals)

A

melting and boiling point decrease
density increase
softness increase
reactivity increase

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7
Q

difference between alkali metal and alkaline earth metal

A

not as reactive as group 1 metals
and form 2+ ions

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8
Q

what are halogens

A

halogens are the most reactive non-metals

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9
Q

which group are halogens in

A

group 7

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10
Q

which ions do halogens form

A

-1

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11
Q

how does reactivity change down the group and why (halogens)

A

reactivity decreases

as the shell number increases the force of attraction between the nucleus and the outer electron decreases, halogens take electrons and don’t give hence making it harder to gain the electron decreasing the reactivity

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12
Q

how does the intensity of the colour change down the group(halogens)

A

colour intensity increases (gets darker)

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13
Q

name the elements and the colours down the group in this group (halogens)

A

flourine/chlorine is greenish-yellow
bromine is orange-brown
iodine is dark brown
astatine is black

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14
Q

how does the melting and boiling point change down the group and why(halogens)

A

increases

as it gets less reactive it is harder to gain an electron
making the bonds harder to break causing there to be a higher temperature needed to break the bonds

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15
Q

how do the states of the elements change in halogens down the group

A

first two elements are gaseous (flourine and chlorine)
bromine is liquid
iodine and astatine are solid

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16
Q

how does density vary down the group

A

density increases

as the mass number increases there will be more particles per unit volume increasing the density

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17
Q

what are noble gases also known as

A

inert gases

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18
Q

how do noble gases react

A

they are unreactive

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19
Q

which group are they in (noble gasses)

A

group 8

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20
Q

how does melting and boiling point vary down this group and why (group 8)

A

increase

as the gases get heavier it is harder to vaporise, causing there to be a need in higher temperature supplied to vaporise the element

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21
Q

how does density vary down the group 8

A

density increases

as the mass number increases there will be more particles per unit volume increasing the density

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22
Q

properties of metals (physical)

A

high density
malleable
ductile
strong
shiny
conductor of heat
conductor of electricity
sonorous
high melting
high boiling

23
Q

chemical properties of metals with oxygen

acidic or basic

A

all metals react with oxygen to form metal oxide (metal oxides are basic in nature)

24
Q

chemical properties of metals with acid

A

metal + acid —> salt + hydrogen

25
Q

chemical properties of metals with water

A

metal + water –> metal hydroxide + hydrogen

some of the metal that doesn’t react with water forms metal oxide + hydrogen

26
Q

transition metal chemical properties

A

variable valencies
compounds of transition metals are coloured
used as catalysts
metal + water –> metal hydroxide + hydrogen
metal + acid —> salt + hydrogen
metal + oxygen –> metal oxide

27
Q

chemical property of metals when reacted with non-metals

A

form ionic compounds

28
Q

which metal is the most reactive with water and what does it form

A

potassium
reacts violently with cold water (catches fire)

products: hydrogen, KOH (K + h2o –> KOH + H2)

29
Q

which metal is the second most reactive with water and what does it form

A

sodium
violent with cold water

products: hydrogen, NaOH (Na + h2o –> NaOH + H2)

30
Q

which metal is the third most reactive with water and what does it form

A

calcium
less violent with cold water

products: hydrogen, calcium hydroxide (Ca + h2o —> Ca(OH)2 + H2)

31
Q

how can we compare metals reactivity

A

reacting them with the same reactant. If one metal is more reactive than the other it will react faster and more vigorously, at a lower temperature

32
Q

which metal is the most reactive with hcl and what does it form

A

magnesium

products: hydrogen, magnesium chloride (Mg + HCl —> MgCl2 + H2)

33
Q

which metal is the second most reactive with hcl and what does it form

A

zinc

products: hydrogen, zinc chloride (Zn + HCl —> ZnCl2 + H2)

34
Q

magnesium displaces hydrogen when reacted with hcl and when reacted with water what does this mean

A

this means magnesium is more reactive than hydrogen and has a stronger drive to give away electrons hence having a stronger drive to form compounds

35
Q

which metal is the most reactive with oxygen and what does it form

A

sodium

products: sodium oxide (white solid) (Na + O2 —> Na2o)

36
Q

which metal is the second most reactive with oxygen and what does it form

A

calcium

products: calcium oxide (white solid) (Ca + O —> CaO)

37
Q

which metal is the third most reactive with oxygen and what does it form

A

magnesium

products: magnesium oxide (white solid) (Mg + O —> MgO)

38
Q

how does the speed of magnesium reacting with water vary

A

reacts with water slowly but vigorously with steam

39
Q

in a metals reactivity series why are non-metals hydrogen and carbon present

A

they are used to extract metals from their oxides

40
Q

state the reactivity series of metals

A

potassium
sodium
calcium
magnesium
aluminium
carbon
zinc
iron
hydrogen
copper
silver
gold

41
Q

list the 4 most reactive metals and their reactions with water (balanced)

A

potassium
2K + 2H2O —> 2KOH + H2
sodium
2Na + 2H2O –> 2NaOH + H2
calcium
Ca + 2H2O –> Ca(OH)2 + H2
magnesium
Mg + 2H2O –> Mg(OH)2 + H2

42
Q

which metals react with steam and not water

A

metals below calcium (magnesium,aluminium,carbon,zinc,iron,hydrogen,copper,silver
gold)

43
Q

which metals will react with dilute acids

A

metals above hydrogen

44
Q

why are some metals more reactive than others

A

This is because more reactive metals lose electrons and form ions more readily than less reactive metals, making them better reducing agents

45
Q

what is rusting

chemical compound of rust

A

Rust is a chemical reaction between iron, water and oxygen to form the compound hydrated iron(III) oxide (which is rust)

46
Q

which compound and element must be present for rusting to occur

A

compound: water
element: oxygen

47
Q

what happens to iron during rusting

A

iron gets oxidised

48
Q

what is the “barrier method” of rust protection

A

Rust can be prevented by coating iron with barriers that prevent the iron from coming into contact with water and oxygen

49
Q

what are common barrier materials that are used

A

grease, oil, paint, plastic

50
Q

which metals can rust, when other metals are broken down in the presence of water and oxygen what is it called.

A

only iron and an alloy of iron can rust

if any other metal is broken down it is known as corrosion

51
Q

how can iron be prevented from rusting other than by using a barrier

A

using a metal that is more reactive than iron causing that metal to oxidise first and corrode

52
Q

what is galvanising

A

Galvanising is a process where the iron to be protected is coated with a layer of zinc

53
Q

how can the layer of zinc be applied on to iron

A

electroplating or dipping it into molten zinc

54
Q

what is formed when zinc reacts with air

A

ZnCO3

55
Q

explain why a metal is/is not suitable as a method of preventing an iron/steel object from rusting.

A

if it is higher in the reactivity series than iron, it will be suitable for sacrificial protection as it will be oxidised instead of iron.

If it is lower in the reactivity series than iron, it would not be suitable as iron would be oxidised, causing it to rust.

56
Q

two ways in which physical properties of transition elements differ from group 1 metals

A

higher density
higher boiling points

Chem (31 decks)

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