Chemistry 3.4 Flashcards
1
Q
Chemical formula of Hydroxide
A
OH -
2
Q
Chemical formula of Nitrate
A
NO3 -
3
Q
Chemical formula of Carbonate
A
CO3 2-
4
Q
Chemical formula of Sulphate
A
SO4 2-
5
Q
Chemical formula of Ammonium
A
NH4 +
6
Q
What does -ate mean?
A
Tells you that oxygen is present.
7
Q
What do acids form when added to water?
A
They form positively charged Hydrogen ions (H +)
8
Q
What do alkalis form when added to water?
A
They form negative hydroxide ions (OH –)
9
Q
metal + acid –>
A
salt + hydrogen
10
Q
metal oxide + acid –>
A
salt + water
11
Q
metal hydroxide + acid –>
A
salt + water
12
Q
carbonate + acid –>
A
salt + water + carbon dioxide
13
Q
Ammonia + acid –>
A
Ammonium salt
14
Q
Formula of Sulphuric acid
A
H2 SO4
15
Q
Formula of Nitric acid
A
HNO3
16
Q
Formula of hydrochloric acid
A
HCl
17
Q
Formula of phosphoric acid
A
H3 PO4
18
Q
When do diatomic atoms apply?
A
When the element is on its own in a symbol equation
19
Q
Are Nitrates soluble?
A
Yes
20
Q
Are halides soluble?
A
Most EXCEPT lead (II) and sliver halides
21
Q
What are halides?
A
Elements in Group 7.
22
Q
Are sulfates soluble?
A
Most EXCEPT lead (II), barium and calcium sulfates.
23
Q
What is the charge on lead (Pb)?
A
2+
24
Q
Which group’s salts are always soluble?
A
Group 1.
25
Are Carbonates soluble?
No, however GROUP 1 CARBONATES ARE SOLUBLE.
26
Are Hydroxides soluble?
No, however GROUP 1 HYDROXIDES ARE SOLUBLE.
27
Are Ammonium salts soluble?
Yes, except ammonium oxides.
28
What is an alkali?
Releases Hydroxide (OH-) ions.
29
What are metal oxides?
Bases.
30
What are non-metal oxides?
Acids.
31
What is an observation of magnesium oxide/combustion of magnesium?
Bright white light or white solid formed.
32
Why is the acid heated up in a reaction?
To speed up the reaction.
33
What is an observation of sulphur dioxide?
Blue flame.
34
Charge on Zinc Iron
2+
35
Charge on Silver ion
+
36
Charge on Copper
2+
37
Charge on Lead
2+
38
Describe how to find out if an unknown element is a metal or non-metal.
Combust with oxygen.
Dissolve the oxide in water.
Determine the pH of the solution with an indicator.
Metal = Alkali solution
Non metal dioxides = Acid solution
39
Methyl Orange Indicator colour change
Red in acid
Orange in neutral.
Yellow in alkalis
40
Steps to prepare lead (II) sulphate
Mix 2 soluble salts together while stirring
Filter to remove precipitate from mixture
Wash filtrate with distilled water to remove traces of other solutions
Leave in an oven to dry
41
Abundance of Nitrogen in air.
78%
42
Abundance of Oxygen in air.
21%
43
Abundance of Argon in air.
0.9%
44
Abundance of Carbon Dioxide in air.
0.04%
45
What is an acid?
A H+ donor.
46
What is a base?
A H+ acceptor
47
What is an alkali?
An OH- donor.
48
What should you be careful with when using polyatomic ions in chemical formulae?
You have to use brackets.
49
Observations of a carbonate + acid reaction.
Carbonate disappears- Is used up in reaction.
Fizzing- Gas (carbon dioxide) is produced.
50
Steps for Insoluble Base method.
1- Heat acid (speeds up reaction)
2- While stirring, keep adding base until no more will dissolve. (Guarantees that all the acid has been used up/excess base)
3- Filter out the excess base
4 - Transfer to evaporating basin
5 - Heat until crystals form on glass rod
6 - Allow solution to cool for a few days
7 - Filter out crystals
8 - Dry crystals using filter paper
51
When would you use the Titration method?
When the base you are using is soluble, the insoluble base method wouldn't work because you wouldn't be able to filter out the excess.
52
Crystallisation - You use this no matter which method you used to make the salt (but only for soluble salts)
1 - Transfer solution to an evaporating basin. Heat the salt solution and stir with a glass rod until crystals start to form (causes solution to become saturated).
2- Allow solution to cool for a few days (reduces solubility of solution).
3- Filter out the crystals.
4- Pat the crystals dry with filter paper.
53
Making an insoluble salt by precipitation method
1- Mix two solutions together in a beaker. (Dissolve in water if they are solid)
2- Filter to collect the solid precipitate.
3- Wash with distilled water.
4- Pat the solid dry with filter paper.
54
What type of solutions do metal oxides form when dissolved in water?
Alkaline
55
What type of solutions do non-metal dioxides form when dissolved in water?
Acid
56
Observation of carbon combusting
Orange glow, universal indicator in water turns from green to orange
57
Observation of iron combusting
Burns very quickly with orange flame, universal indicator in water turns from green to dark green
58
What are all metal oxides and hydroxides?
Bases
59
Reasons for why the % of oxygen in air experiment result does not match.
Leaks in equipment letting more air (and therefore oxygen) into the experiment.
Metal wasn't heated enough or for long enough for all the oxygen to react
60
What do all bases react with acid to form?
salt and water
61
Why is Ammonia (NH3) a base?
Can accept H+ to form ammonium ion
62
What is an alkaline solution?
Alkali has dissolved and donated OH- into the water causing a pH greater than 7
63
Observation of Hydrogen combusting
Squeaky pop
64
What is produced when hydrogen is combusted?
Water
