1.2 The Periodic Table Flashcards
(17 cards)
1
Q
Groups
A
- Columns in periodic table.
- Same number of electrons in outermost shell.
- Similar chemical properties.
2
Q
Periods
A
- Rows in periodic table.
- Same number of shells.
3
Q
Location of metals and non-metals in periodic table.
A
- Metals: left and bottom
- Non-metals: right and top.
4
Q
Why is the table called a periodic table?
A
Similar properties occur in regular intervals
5
Q
Problems with early periodic table.
A
- Ordered in atomic weight - did not consider isotopes.
- Incomplete
- Some elements placed in inappropriate groups.
6
Q
How did Mendeleev order the periodic table?
A
- Ordered in atomic weight.
- Switched order of some elements so they fit the properties of other elements in their group.
- Left gaps for undiscovered elements and predicted their properties.
7
Q
Group 1 name
A
Alkali metals.
8
Q
Group 1 properties
A
- Soft
- Low MP and BP (compared to other metals).
- Low density (float on water)
- Highly reactive
- Ionic reaction with halogens to form ionic compounds (salts)
9
Q
Group 1 reaction with oxygen
A
Metal + oxygen -> metal oxide
10
Q
Group 1 reaction with water
A
Metal + water -> metal hydroxide + hydrogen
- Metal hydroxide = alkaline (test with indicator)
- Hydrogen = lit splint ignites with squeaky pop.
11
Q
Group 1 reaction with chlorine
A
Metal + chlorine -> metal chloride
- Metal chloride = white solid.
- Chlorine = green gas.
- Exothermic = bright light produced as green gas disappears.
12
Q
Group 1 progressive reactivity.
A
- Reactivity increases as you go down the group.
- The atoms have more shells.
- The distance between the outer shell and nucleus increases.
- There is a weaker magnetic attraction between the positive nucleus and negative outer electrons.
- There is more shielding from inner electron shells.
- It is easier to lose an electron to become stable.
13
Q
Group 7 name
A
Halogens
14
Q
Group 7 properties
A
- Diatomic molecules.
- Coloured vapours.
- MP and BP increase down the group (solid to gas) - more intermolecular forces to break between shells.
- Displacement reactions in aqueous solutions of its salt.
- Ionic reaction with metals to form ionic compound.
- Covalent reaction with non-metals to form covalent compounds.
15
Q
Group 7 progressive reactivity.
A
- Less reactive as you go down the group.
- The atoms have more shells.
- The distance between the nucleus and outer-shell increases.
- The magnetic attraction between the positive nucleus and negative outer electrons weakens.
- There is more sheilding from inner electron shells.
- It is harder to gain an electron to become stable.
16
Q
Group 0 name
A
Noble gases
17
Q
Group 0 properties
A
- (MP and) BP increases down the group - more intermolecular forces needs more energy.
- Un reactive and don’t usually form molecules - stable electron arrangements.
