Ch 2 - Periodic Table Flashcards
(114 cards)
1
Q
Who made the law of octaves?
A
Newlands.
2
Q
Who created a spiral to show the elements in order of atomic weight?
A
Chancourtois.
3
Q
Who’s periodic table is most similar to the table we use now?
A
Mendeleev’s.
4
Q
What are the group of elements in the middle of the periodic table called?
A
Transition metals.
5
Q
In group 1 (the alkali metals) what is the most reactive element?
A
Francium.
6
Q
What is the name of the elements in group 7 called?
A
The halogens.
7
Q
In group 7, are the elements more reactive at the top of bottom of the column?
A
At the top.
8
Q
As you go down group 1, what happens to the melting points of the metals?
A
It decreases.
9
Q
Are alkali or transition metals used in a catalyst?
A
Transition metals.
10
Q
Why was Mendeleev’s periodic table not accepted at first?
A
He had not discovered all the elements in the table and he swapped some elements around that other scientists did not agree with.
11
Q
Which produce more colourful salts, transition or alkali metals?
A
Transition metals make colourful salts
12
Q
What is a halogen?
A
An halogen is an element from group 7
13
Q
What is an halide?
A
A compound including a halogen
14
Q
Do alkali metals have a high or low density?
A
They have a low density compared to transition metals.
15
Q
Do group 1 metals have high or low boiling/melting points?
A
They have low boiling/melting points
16
Q
How many electrons do alkali metals have on their highest energy level?
A
They have one electron on their outer shell
17
Q
As you descend group 1 they react more quickly with air, true or false?
A
True, as you descend group 1 they react more quickly with air
18
Q
Why are the Metals in group 1 Called Alkali metals?
A
Because they all form hydroxides which hissolve in water to give strongly alkaline solutions
19
Q
Why Are alkali metals Stored in Oil?
A
To prevent Them From reacting with the oxygen in the Air
20
Q
Why wasn’t John newlands theory widely accepted?
A
Because he was forced to put elements in the same groups as other elements even if their properties weren’t similar. For example he put iron in the same group as oxygen
21
Q
How did mendeleev order his elements in his table?
A
By atomic mass
22
Q
What made mendeleevs table so clever?
A
He knew where gaps were in the table and so predicted what properties the elements would have once they were discovered.
23
Q
Why did mendeleev’s table gain credit after his table was published?
A
Because the properties of new found elements fit in with his predictions.
24
Q
How did mendeleev overcome the problems newlands had faced?
A
He swapped elements around In some circumstances so that the properties were similar
25
What happens as you go down the list of alkali metals?
They become more reactive
26
Why are the noble gases unreactive?
Because they have a full outer shell
27
How many groups are there in the periodic table?
18
28
What happens as you go down the list of halogens?
They become less reactive
29
What was John newlands theory called ?
The law of octaves
30
A more reactive halogen will do what to a less reactive halogen in a halide solution?
It will displace it
31
Why do the element get less reactive as we move down group 7?
Because there are more electrons rings, which are therefore further away from the nucleus. As a result there is a weaker attraction towards the nucleus and therefore harder to gain an electron- less reactive.
32
What type of reaction includes a non-metal and a metal?
Ionic bonding
33
Chlorine, hydrogen, oxygen and nitrogen are all what?
Diatomic elements
34
What did Meyer not include in his version of the periodic table?
Transition metals
35
In what way was Mendeleev limited in order to produce the periodic table?
Only 60 element had been discovered
36
Who called there idea "telluric spiral"?
Chancourtois
37
Why where other scientists critical of Newlands' Law of Octaves?
Non-metals and metals were mixed together. He put more than one elements in each box.
38
As you work down the group 1 metals, how do their boiling points change?
They decrease.
39
Do transision metals form coloured or non coloured compounds?
Coloured
40
Do transision metals have high or low melting points?
High
41
Are transition metals useful catalysts?
Yes
42
What happens to the reactivity of the halogens as you go down the group?
They become less reactive
43
What happens to the reactivity of the atom as you go down group 1?
They become more reactive
44
Which group is sodium in?
Group 1
45
Which group are atoms with one electron on the outer shell in?
Group 1
46
Which scientist came up with a table that used the law of triads?
Johann Döbereiner.
47
What is the name of each vertical column in the periodic table we use today (a variation of Mendeleev's)?
A group.
48
How are elements arranged on the periodic table we use today (a variation of Mendeleev's)?
By increasing atomic number.
49
What is the name of each horizontal row in the periodic table we use today (a variation of Mendeleev's)?
A period.
50
What do elements in the same group share?
Similar properties.
51
What is the name of group 1?
The Alkali metals.
52
What is the name of group 7?
The Halogens.
53
What is the name of group 8?
The Noble gases.
54
Which metals form ionic compounds on reaction with non-metals
Alkali and transition
55
Which metals have a low density?
Alkali metals
56
Which metals have high melting points?
Transition metals
57
Which metals are used as catalysts?
Transition metals
58
Which metals compounds dissolve in water to give colourless solutions?
Alkali metals
59
Do alkali metals have low or high melting points?
Low melting points
60
Do all atoms become more reactive with more electron shells?
No, the Halogen gases become less reactive as they descend the table.
61
Which six elements commonly travel in pairs?
Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine
62
Which element does not fit in the periodic table?
Hydrogen
63
What changes as we go across the periodic table?
The amount of electrons on the outer shell.
64
What changes as we go down the periodic table?
The number of electron shells.
65
What is a group?
Elements in the column
66
What is a period?
Elements in a row
67
Where are metals in the periodic table?
On the left and middle
68
Where are non metals in the periodic table?
On the right
69
Are metals electrically conductive?
Yes
70
Are non metals electrically conductive?
No
71
Are metal oxides acid or alkali?
Alkali
72
Are non metal oxides acid or alkali?
Acid
73
Why do elements in the same group of the periodic table have the same chemical properties?
Because they all have the same number of electrons in their outer shell and therefore give away or gain the same amount of electrons when they react with another element
74
What are the noble gases?
A group of inert gases
75
Why are noble gases extremely unreactive?
Because they all have a full outer shell of electrons and therefore have no need to gain or lose any electrons by reacting with another element
76
Describe the reaction of lithium with water
Lithium doesn't melt but fizzes on the surface of the water and produces an alkaline solution
77
Describe the reaction of sodium in water
Sodium melts into a small ball on the surface of the water giving of hydrogen, producing an alkaline solution. Sodium catches fire with an orange flame on filter paper on top of the water.
78
Describe the reaction of potassium with water
Potassium melts giving off hydrogen which catches fire with a LILAC flame producing an alkaline solution.
79
How does the melting/boiling point of the group 1 metals change as you go down?
It decreases, i.e. Lithium is highest
80
How does the density of group 1 metals change as you go down the group?
It increases, i.e. lithium is least dense
Think about how lithium sodium and potassium are all less dense than water and float on it
81
How should you store group 1 metals and why?
Lithium, sodium and potassium should all be stored on oil because they all react quickly with air to form oxides and violently with water.
Rubidium and caesium are so reactivw that they have to be stored in a sealed glass container to stop any possibility of oxygen getting to them.
82
What colour are group 1 metal ions?
And so what colour are their compounds?
colourless
colourless or white unless they are paired with a coloured negative ion
83
How does the reactivity change as you go further down the group 1?
The elements become more reactive as you go further down the group
84
In conclusion group 1 elements:
| (8)
* are metals
* are soft with melting points and densities that are very low for metals
* have to be stored out of contact with air and water
* react rapidly with air to form coatings of the metal oxide
* react with water to produce an alkaline solution of the metal hydroxide and hydrogen gas
* increase in reactivity as you go down the group
* form compounds in which the metal has a 1+ ion
* have mainly white compounds which dissolve to produce colourless solutions
85
What are the alkali metals?
Group 1 metals
86
Why do elements in group 1 get more reactive as you move further down the group?
Because the outer electron is further from the nucleus which means the attraction between the nucleus and electrons is less and so the electron is more easily lost.
87
What is the colour and state of chlorine at room temperature?
Green gas
88
What is the colour and state of bromine at room temperature?
Brown liquid
89
What is the colour and state of iodine at room temperature?
Grey solid
90
Predict the properties of other halogens in this group
Black/grey solid 7 outer shell electrons Less reactive than other halogens
91
How does the reactivity change in group 7?
Elements become less reactive as you go further down the group
92
Why do elements in group 7 become less reactive as you go further down the group?
Because it's harder to gain an extra electron because the outer shell is further from the nucleus and so there is less attraction.
93
How are the halogens dangerous?
Fluorine is extremely reactive.
They all have very poisonous vapours and so should be handled in a fume cupboard.
Liquid bromine is corrosive
94
Describe an experiment to show that a more reactive halogen will displace a less reactive halogen and form a solution of one of its salts.
Sodium bromide + chlorine = sodium chloride + bromine
Sodium iodide + chlorine = sodium chloride + iodine
95
Make this equation into an ionic equation 2Na+ + 2Br- + Cl2 = 2Na+ + 2Cl- + Br2
2Br- + Cl2 = 2Cl- + Br2
96
What are these displacement reactions known as?
Redox reactions
97
In the reaction with sodium bromide and chlorine which element has been oxidised and which one has been reduced?
Bromide has been OXIDISED Chlorine has been REDUCED
98
What is the atomic number?
The number of protons in the atoms of the element.
99
Physical noble gas properties
The noble gases are all colourless, monatomic gases; this means their molecules consist of single atoms.
100
Differences between metals and non-metals
Metals conduct electricity and heat Are shiny when polished and malleable Usually solids with high melting points Oxides which are alkaline Poor conductors of heat, don't usually conduct electricity Have oxides which are acidic or neutral Usually brittle as solids Tend to have low melting and boiling points
101
What happens to the melting point of group 1 metals as you go down the group?
Gets lower
102
Why are group 1 metals stored in oil?
Because they react with water vapour and oxygen in the air.
103
What does it mean if there are bubbles in a beaker of oil containing a group 1 metal?
There must have been a tiny bit of water in the oil.
104
What is the periodic table arranged in the order of?
The atomic (proton) numbers of the elements.
105
What colour are the compounds of group 1 elements usually?
White or colourless
106
Fluorine at room temp
Yellow gas
107
why must you be careful with halogens?
They have coloured poisonous vapours.
108
LEARN HOW TO DRAW A METAL STRUCTURE AND ALL THE DIAGRAMS
Ugh ok fine
109
In conclusion group 7 elements:
| (7)
* Have diatomic molecules, X2
* Go from gases to liquid to solid as you move down the group
* Have coloured, poisonous vapours
* Form ionic salts with metals and covalent compounds with non-metals
* become less reactive as you go down the group
* are oxidising agents with oxidising ability decreasing down the group
* will displace elements lower down the group from their salts
110
Generally, what are the properties of the transition metals?
All typically metallic elements
good conductors of heat and electricity
Workable, strong and mostly with high densities
With the exception of liquid mercury they all have fairly high to very high melting points
111
are transition metals more or less reactive than group 1 metals?
much less reactive and so they don't react as rapidly with air or water
112
What are the physical properties of the compounds of transition elements?
They usually form coloured compounds
113
Transition metals are often useful catalysts, name 3 useful transition metals and their compounds that are useful catalysts:
* iron in the manufacture of ammonia
* vanadium (V) oxide, V2O5, in the manufacture of sulfuric acid
* manganese (IV) oxide, MnO2, in the decomposition of hydrogen peroxide.
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