Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry IGCSE > Chapter #13 - The Periodic Table > Flashcards

Chapter #13 - The Periodic Table Flashcards

forgot unit number and name

1
Q

What is similar in the electron configuration of group 1 metals?

A

They all lose one electron.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the observations of Li at room temp?

A

Grey solid (stored in oil to prevent reaction with oxygen and water).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the observations of Li with water?

A
  • Effervescing
  • Li disappears
  • temp. increase
  • floats and moves on surface
  • Produces colorless solution
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the observations of Na at room temp.?

A

Shiny silver soft solid. (Like a block of cheddar)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the observations of Na with water?

A
  • Effervescing
  • Na disappears
  • Temp. increase
  • Floats and moves on surface
  • Produces colorless solution
  • Melts and forms a sphere
  • If prevented from moving, ignites with yellow/orange flame.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the observations of K at room temp.?

A

Very easy to cut (soft), grey solid, when cut, inside shiny.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are the observations of K with water?

A
  • effervescing
  • K disappears
  • Temp. increases
  • Floats and moves on surface
  • produces colorless solution.
  • Melts and forms a sphere
  • Ignites with lilac flame
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Which way are group 1 metals more reactive?

A

The group 1 metals become more reactive descending the group.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

why are group 1 metals more reactive descending the group?

A

Because the outer electron is further from the nucleus. therefor, there is weaker electrostatic force of attraction, less energy is needed to remove the outer electron.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What reactivity depend on in metals?

A

Their ease to lose an electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What way do group one metals have a higher mpt.?

A

The mpt. of group 1 metals increases while going up the group.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the density of group 1 metals?

A

All group 1 metals have low densities.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What color and state of matter are ALL group 1 compounds?

A

They are ALL white solids.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are the observations of lithium chloride in water?

A

dissolves (not much)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are the observations of sodium carbonate with water?

A

dissolves (not much)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are the observations of potassium chloride with water?

A

dissolves (not much)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the observations of lithium chloride when it reacts with oxygen (with flame)

A

Makes red flame (does not melt)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are the observations of sodium carbonate when it reacts with oxygen (with flame)?

A

Makes a orange/yellow flame

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are the observations of potassium chloride when it reacts with oxygen (with flame)?

A

Makes a lilac flame.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are group 1 metals called?

A

alkalimetals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are three things group 1 metal compounds have in common?

A
  • White solids
  • Produce colorless solution (with water)
  • Soluble in water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What are group 7 elements called?

A

Halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What elements are diatomic?

A

Halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does diatomic mean?

A

The elements exist in pairs (X2)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
What colors is fluorine in its viable states? What is its standard form?
Solid: X Liquid: X Gas: pale yellow* (aq): colorless
24
What colors is chlorine in its viable states? What is its standard form?
Solid: X Liquid: X Gas: pale green* (aq): pale yellow
25
What colors is bromine in its viable states? What is its standard form?
Solid: X Liquid: red/brown* Gas: orange (aq): orange
26
What colors is iodine in its viable states? What is its standard form?
Solid: grey* Liquid: X Gas: purple (aq): orange/brown
27
What way do group 7 non-metals have a higher mpt. and why is this?
Group 7 metals have a higher mpt. going down. This is because the atom (and molecules) increase in size. Therefore there are more IMFs so more energy is required to break them apart.
28
What is test 1 and test 2 for chlorine?
Test 1: damp blue litmus => red =>white Test 2: add hexane => colorless
29
What is test 1 and test 2 for bromine?
Test 1 => damp blue litmus => red => white (but slower than chlorine) Test 2 => add hexane => orange
30
What is test 1 and test 2 for iodine?
Test 1: add starch => blue/black Test 2: add hexane => pink
31
What happens to the colors in group 7 moving down?
They get darker.
32
What is the explanation for test 1 (damp blue litmus paper)of chlorine?
Cl2 + H2O => HCl + HOCl HCL= Hydrochloric acid (red) HOCl => chloric acid (bleach)
33
What is the explanation for test 1(damp blue litmus paper) of bromine?
Br2 + H2O => HBr + HOBr HBr = hydrobromic acid HOBr = bromic acid
34
What is the reaction of chlorine with iron? What are the states of matter and color of each substance? What happens as the reaction occurs?
iron + chlorine => iron (III) chloride 2Fe + 3Cl2 => 2FeCl3 Glows red as reaction happens Fe= grey solid Cl2= green gas FeCl3 = brown solid
35
What is the reaction of bromine with iron (only symbol equation)? What are the states of matter and color of each substance? | How does it's reactivity compare to chlorine
3Fe + 3Br2 => 2FeBr3 bromine is less reactive than chlorine
36
What way do group 7 non-metals have a lower reactivity and why?
Group 7 non-metals reactivity decreases going down the periodic table.The lower you go in the group, the more occupied elements the atoms have, therefor, the nucleus gets farthre away from the electron it needs to attract and so it has a weaker electrostatic force.
37
What is the definition of displacement in chemistry?
A more reactive element replaces a less reactive one from a compound.
38
What is displacement of halogens? (In my own words)
A more reactive halogen (group 7 non-metal) replaces a less reactive halogen in a compound with a metal.
39
What are halides?
Ions of group 7
40
What do you call ions of group 7?
Halides
41
What are group 2 metals called?
Alkaline earth metals
42
What are alkaline earth metals?
Group 2
43
What way do group 2 metals decrease in mpt. ? | How does it compare to group 1
The mpt. decreases as it goes down the periodic table.This is because the electrostatic forces get weaker as you go down the row. But, the mpt. of any group 2 atom will be higher than any group 1 atom. This is due to higher magnitude of charge and more delocalized electrons.
44
What way are group 2 metals more reactive? | and how does that compare to group 1
The reactivity increases going down, but less reactive than group 1 as they need to lose 2 electrons.
45
What are the properties of transition metals?
* High mpt. (higher than 1 & 2) * High density * Variable charges (2+, 3+ => 8+) (can change on what it is reacting with and how much energy is present) * Form color compounds * Acts as a catalyst
46
What is the color of the ion Fe^2+
Green
47
What is the color of the ion Fe^3+
Orange
48
What is the color of the ion Cu^2+
Blue
49
What is the color of the ion Mn^7+
Purple
50
What is the color of the ion Cr^3+
Green
51
What is the color of the ion Cr^6+
Orange
52
What is group 8 called?
Noble gases (0)
53
What are noble gases (0)?
Group 8
54
What are some of the characteristics of noble gases?
* Full outer energy level => unreactive/inert * NO bonding exists as single atoms (discrete)
55
What are the properties of noble gases?
* Very low mpt. , very weak inter-atomic forces. Mpt. increases He=>Ar * Do not conduct because they have no charged particles. * Insoluble in water
56
What are the uses of He?
Balloons/air ships (less dense than air)
57
What are the uses of Ne?
Lighting (produces color with electricity)
58
What are the uses of Ar?
Lightbulbs (inert atmosphere)
59
Metal + Oxygen =>
Metaloxides
60
Metal oxide + water =>
Metal hydroxide
61
What happens after metal oxides and water react?
They dissociate (if they are soluble). That is why when you add universal indicator, and the solution is soluble, chemicals have already separated, so the acids and base ions are separated from the metal ions.
62
What is Li + O2? Right the WHOLE equation and balance it. State of matters? Reaction? Colors?
4Li + O2 => 2LiO Burns with red flame Li = Grey (s) O2 = Colorless (g) Li2O = White (s)
63
What is Li2O with water? Colors? State of matters? U.I. added? Sloubility?
* Li2O + H2O => 2LiOH * Li2O = white (s) * H2O = colorless (g) * LiOH = colorless (aq) * Turns purple with U.I. (OH ion is strong base)
64
What is Mg with oxygen? Color? Reaction? States of matter?
* 2Mg + O2 => 2MgO * Mg = grey (s) * O2 = colorless (g) * MgO = white (s) * Forms white flame
65
What is MgO with water? Color? Soluble? States of matter? Color with U.I.?
* MgO + H2O => Mg(OH)2 * Makes white suspension * Dissolves very little * Add U.I. = Blue (weak acid)
66
What is Ca with oxygen? Color, States of matter ect.
* 2Ca + O2 => 2CaO * Ca = grey (s) * CaO = white (s) * Burns with brick-red flame | If you are confused, review notes on metal oxides
67
What metal oxides don't react with H2O?
* Al2O3 * Fe2O3 * ZnO | If you are confused, review your notes on metal oxides
68
What is the product of non-metals and oxygen?
Covalent(non-metal) oxides with a discrete structure
69
non-metal oxide + water =>
acid
70
What does exothermic mean?
Releases a lot of heat
71
What is the general state of metal oxides at room temp.?
Solids | Generally, sometimes they arn't, but in those instances, you can not tel
72
What is the general state of non-metal oxides and
Gases
73
What is the general pH of metal oxides?
<7 (bases)
74
What is the different rule for when you write the product of a non-metal + water?
You have to write the prefix before each chemical to know how much there is of each chemical.
75
Write the prefixes from 2-7
Di = 2 Tri= 3 Tetra = 4 Penta = 5 Hexa = 6 Hepta = 7
76
What is the symbol equation of phosphorus + oxygen and what are some of the things that happen?
4P +5O2 => 2P2O5 (diphosphourupent(a)oxide) * It spontaeneously combusts with a white flame when it reacts. * Product has a high(ish) mpt. even though it is covalently bonded. This is beacuse it has a lot of IMF's because it is a large molecule.
77
What is the equation for diphosphourouspentaoxide + water => and what happens?
P2O5 + 3H2O => 2H3PO4 * When the reaction happens it is exothermic * It make phosphoric acid * It makes a *really* strong acid pH = 0
78
What are the chemicals in the air and how what perecntage of the air do they make up?
* Nitrigen (78%) * Oxygen (21%) * Argon (0.97%) * Carbon dioxide (0.03%)
79
What are the properties of transition metals?
* High mpt. (higher than group 1+2 metals * High density * Variable charges (2+, 3+...8+) Can change depending on what it is reacting with and how much energy is present. * Form color compunds
80
# Compared to group 1 metals What are the mpt. of alkaline earth metals?
Always higer than geoup 1 metals - due to higher magnitude of of charge and more delocalized electrons.
81
What way do group 2 metals have a lower mpt.
Going down the periodic table
82
What way do group 2 metals decrease in reactivity.
They decrease in reactivity going up. But it is less reactive than group 1 beacuse they have to loes to electrons.
83
Are group 1 or group 2 atoms bigger?
Group 1 atoms are bigger.
84
What color is any lithium flame (generally)?
Red flame
85
What color is any sodium in a flame (generally)?
Orange/yellow
86
What color is any potassium in a flame (generally)?
Lilac
87
What is CaO with water? Color, recation, U.I. ect.
* Ca + H2O => Ca(OH)2 * White suspension * dissolves only a little * Add U.I. => blue (weak base - a little stronger the Mg(OH)2)
88
What is Al with oxygen?Also what happens when you add U.I to product?
4Al +3O2 => 2Al2O3 Burns with orange flame
89
Fe with oxygen only need color and the clarification. write the symbol equation but also the product in words. | Does the product dissolvein water?
* 4Fe + 3O2 => 2Fe2O3 * Fe2O3 = Iron (III) oxide * Fe2O3 = Orange /brown * The product does not dissolve and U.I does not work on it beacuse U.I. only works on solutions.

Chemistry IGCSE (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions