Year 10 term 1 Flashcards
(147 cards)
1
Q
Metal + non metal=(what kind of bonding?)
A
ionic bonding
2
Q
Non metal+non metal=(what kind of bonding?)
A
covalent bonding
3
Q
Acid+metal=??
A
Salt+H
because e.g: HCL+Na—>NaCl+H
4
Q
Halogen+metal=???
A
salt. E.g= Cl+Na=NaCl
5
Q
Acid+Base=???
A
neautrelize so: Salt+H2O
E.G=HCL+NaOH—>NaCL+H2O
6
Q
Acid+Carbonate=???
A
Salt+H2O+CO2 E.G=CaCO3
7
Q
Hydrochloric Acid
A
HCl
8
Q
Sodium Hydroxide
A
NaOH
9
Q
Potassium Hydroxide
A
KOH
10
Q
NH4
A
Ammonium
11
Q
Ammonia
A
NH3
12
Q
Phosphoric acid
A
H3PO4
13
Q
Acetic Acid (vinegar)
A
CH3COOH
14
Q
Nitric acid can aka….
A
Hydrogen Nitrate
15
Q
Which of the 3 steel types can be used for surgical tools? Why?
A
Stainless steel-as its highly hygienic.
16
Q
Which of the 3 steels is harder the more carbon there is?
A
High carbon steel-but also less ductile and malleable.
17
Q
Which of the 3 steels is least prone to rusting? Why?
A
Stainless steel- is used for kitchen sinks because of this as the chromium oxide forms a layer atop the iron. Protecting it.
18
Q
Sulphuric acid can aka….
A
Hydrogen Sulphate
18
Q
Nitric acid/Hydrogen Nitrate
A
HNO3
19
Q
Sulphuric acid/Hydrogen Sulphate
A
H2SO4
19
Q
2 bases (hydroxide bases) and formulas
A
Sodium Hydroxide(NaOH) and Potassium Hydroxide(KOH)
20
Q
2 acids+formulae
A
HCl-hydrochloric acid
H2SO4-Sulphuric acid
21
Q
vinegar
A
(CH3COOH) acetic cid
22
Q
Define ‘Metal oxide’
A
metal thats reacted with oxygen
23
Aluminium Ore
Bauxite
24
Hematite compound contains:(chemical formula)
Fe2O3
25
Magnetite compound contains:(chemical formula)
Fe3O3
26
Galena compound contains:(chemical formula)
PbS
27
Copper and below is found as____ in Earths crust
Native or 'free' metals
28
How to extract metals above carbon? Why?
Electrolysis- since they cannot be displaced from their compounds by a less reactive Carbon.
29
Extract metals from there ores below carbon? Why?
Blast furnace/displacement of compound-since carbon is more reactive it will displace the compound giving us the metal and CO2(a waste gas)
30
3 charges of a blast furnace?(chemical compounds and names)
Limestone(Ca2CO3), Coke(impure carbon), hematite(often has sand+Fe2O3)
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Define Ore
When a metal oxide reacts with oxygen and other metals, forming a compound that we call a mineral, contains a valuable metal, we refer to it as an ore. Ores are essentially minerals combined with these metal compounds.
32
Define Native
'free' or uncombined metals.(less reactive metals are usually found free.)
33
Define electrolosis simply. With the ore NaCl
-Molten Na+ ions and Cl- ions in the electrolyte liquid.
-Na+ ions float towards the negative cathode.
-Cl- ions float towards positive anode.
- Cl- gets discharged.
- e- from Cl- flow from cicuit to Na+.
-Na+ recieves e- and becomes reduced.
-Cl floats off as waste and Na is left.
34
What are the 2 rods in electrolysis made of?
Graphite(Carbon)
35
The anode is the____ rod
positive
36
The cathode is the ____ rod
negative
37
Cations ___ their e- to become ____ charged
1. loose
2. positive
38
Anions ___ their e- to become ____ charged
1. gain
2. negatively
39
What is the waste material of using a blast furnace to seperate iron?
SLAG
40
How does a blast furnace work?
The charges are fed at the top (coke,limestone,hematite).
Coke reacts with oxygen and becomes a stronger reducing agent .
CO2 reacts with hematite
Hematite is reduced.
Sand from hematite reacts with limestone to form SLAG. and falls to the bottom on top of the molten iron.
41
# alloys
2 uses of mild steel
car bodies and nails
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# alloys
2 uses of high carbon steel
Knives and cutlery
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# alloys
2 uses of stainless steel
surgical tools and kitchen sink.
44
# alloys
How come alloys are stronger than pure metals?
The different sizing of elements in an alloy make it harder for the atoms to slide off in layers. Much unlike they easily would in a pure metal.
45
# blast furnace extraction method
define coke and its use as a charge in blast furnace.
Coke is impure carbon and reacts with oxygen to become a stronger reducing agent(take oxygen from Iron)
C+O ----> CO2
46
Use of limestone charge in blast furnace?
Limestone undergoes thermal decomposition to also form CO2, another reducing agent
CaCO3 ---> CO2+CaO
47
After limestone undergoes thermal decomposition and coke reacts what happens with the 2 reducing adgents before they actually reduce iron ore?
React with more coke and make carbon monoxide
CO2 + C ----> 2CO
48
What happens to remaining limestone from forming a reducing agent(CO2)?
Reacts with sand to form Slag(Calcium silicate)
CaO+ SiO2 ---> CaSiO3
49
Scientific name and chemical formula for Slag made in furnace?
Calcium silicate
CaSiO3
49
Why do we use molten cryolite in electrolysis?
It **can bring the MP of the metal down**. For e.g: Aluminium usually melts at 2000 degrees C but cryolite reaction can decrease that to 1000 degrees C, so it **economically benfits us**
50
# ore extraction
2 main cost factors of ores
-cost of energy
-cost of reducing agent.
51
define alloy
mixture of metal with carbon or other metal
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Iron and carbon alloy is called...
Steel
53
Why are alloys stronger than pure metals?
Their ***lattice*** structure makes it harder for them to slide over each other
54
How does aluminium alloy resist corrosion?
aluminium oxide forms a layer on top of the surface preventing corrosion
55
Mallable means?
Moldable
56
Ductile means?
can be drawn into a wire.
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advantages of aluminium alloy
is stronger and less dense(lighter), corrodes less easily.
58
mild steel is ---x ---- dense than aluminium alloy
3x more
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range of carbon in high carbon steel? what does this effect?
0.6-1.5%- the more carbon the more resistant and hard but also less malleable and ductile
60
Why does the charge of an atom change once its and ion in terms of protons and electroncs?
In the nucleus we have protons and outside in shells we have electrons, they are the same number in quantity and balance out. therefore if i loose an e- there are more protons which are positive giving a positive charge, and vice versa.
61
define electronegative.
How badly an atom needs electrons.
62
ionic bonding can only take place between a ---- **-** ----- and a ----
non-metal and metal
63
What do periods tell us in periodic table about the atom structure?
The valence shells
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Ammonium ion
| (symbol equation)
NH₄⁺
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Why is ammonium ion positively charged in terms of contents?
It forms when NH3+ gains a hydrogen becoming NH4+ , the protons outweight he electrons.
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Carbonate ion
| (symbol equation)
CO₃²⁻
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Hydroxide ion
| (symbol equation)
OH –
68
sulphate ion
| (symbol equation)
SO₄²⁻
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Nitrate ion
NO⁻ ₃
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Charge of silver ion?
Ag- +1
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Lead ion charge
Pb2+
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Copper ion charge
Cu2+
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Zinc ion charge
Zn2+
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Why are ions formed?
| what force?
Electrostatic force between ions, (metal)+ and (non-metal)- attract.
E.g: Mg+ and Cl- = electrostatic forces make the 2 bond.
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positive ions are called...
Cations
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Negative ions are called..
Anions
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Ionic bonding is....
The electrostatic force between the positive and negative ions.
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List properties of ionic compounds
| atleast 4
- High melting and boiling points
- Insoluble in organic solvents
- Soluble in water
- Crystaline
- Cannot conduct electricity when solid
- Can conduct electricity when molten or in water
79
Why can't ionic compounds conduct electricity when solid?
They don't have free electrons to carry the charge/heat. they do get them when molten or dissolved.
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water is a --- molecule, therefore when we dissolve an ionic compound; the ---- are attracted to the ----- molecules resulting in oxygen being slightly more negative and hydrogen more positive. Now the molecule is called ---- due to the strong forces between water molecules and ions being able to provide energy to break lattice, not all ions can be dissolved though, like ---O
1. covalent
2. electrons
3. Oxygen
4. polar
5. MgO
81
2 things ionic lattice tells us?
| 2 ionic properties
- High melting and boiling points, to break electrostatic bonds
- Brittle- if we slide a negative over a negative and charges resists will result in breakage.
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What do ionic compunds exist as?
Lattice structures
83
Example of organic solvent
ethanol
84
The only 2 ways any substance can conduct energy is if..
1. contains charged particles
2. Particles are free to move
85
The word particles can relate to 2 things, these are...
- ions
- electrons
86
Covalent bonding; metal or non-metals?
Non-metals
87
The electrostatic charges in covalent bonding are the negative ---- attracting to the positive ---- of the other atom.
1. electron
2. nuclei
88
How can an atom gaina nd loose electrons but stay the same element? E.g: Hydrogen gaining an e- doesn't become hellium?
As the number of protons determines which atom it is.
89
Whenever a bond is formed ----- is released, More bonds atoms can form, more ---- is released, more stable the atoms, as when --- is released, the atoms get a lower ---- rate.
1.energy
2.energy
3.energy
4.energy
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Since the covalent bond of N3 is a --- bond, it requires more ---- to break, therefore a N3 is relatively unreactive.
1. triple covalent
2. energy
91
Electrostatic forces in ionic bonding
The positive and negative ions are attracted to each other.
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Electrostatic forces in covalent bonding
Negative electrons attracted to positive nuclei of other atom, they share an electron pair this way and are very strong.
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Electrostatic forces in metallic bonding
Positive atom ion attracts to delocalized electron, this prevents the positive atom ions repelling each other.
94
What is an intermolecular force?
The force between molecules - what we break in covalent molecular bonds when heating
95
Name some covalent giant compounds
- Diamond
- graphite
- SO4
96
# covalent bonding(giant structures)
Structure of a diamond
Tetrahedral arrangmnt- a carbon atom is bonded to 4 other carbon atoms, arranged in a structe where no layers are present.
97
Properties of a diamond
- High MP and BP
- Hard and strong
- Arranged in tetrahederal arrangement
- doesnt conduct electricity
98
Properties of C60 fullerene
- Low MP and BP
- doesnt conduct electricity
- Not as hard as diamond
99
name 3 allotropes of carbon
- C60 Fullerene
- Diamond
- Graphite
100
The only carbon allotrope that can conduct electricity is...
Graphite-has one free electron per carbon atom as bonded in 3 sigma bonds.
101
What is an allotrope?
Different form of the same element- atoms are just arranged differently.
102
# Giant covalent structures
Describe Graphite structure
Hexagonally arranged, 3 sigma bonds per atom and arranged in layers
103
Properties of graphite allotrope
- High MP and BP
- can conduct electricity
- Soft layers slide off each other
104
define discharged in electrolysis
When the ion gains or looses electrones at the electrode, to become stable and is released.
105
Electrolysis in 3 words
decomposition via electricity
106
Ethane, Ethene, and methane
| (chemical formulas)
C2H6, C2H4, CH4
107
Name 4 acid and alkali indicators?
Universal indicator, Litmus, Methyl orange, Phenolphthalein
108
What is the range for strongly acidic solutions(on pH scale) and name one.
0-3, HCl acid
109
Name a weakly acidic solution and give the range for them.(on the pH scale)
4-6, Vinegar( ethanol acid solution)
110
What is the range for strong base solutions(on pH scale) and name one.
8-10, ammonia solution
111
What is the range for weak base solutions(on pH scale) and name one.
11-14, sodium hydroxide solution
## Footnote
most of the time, bases are metal oxides or hydroxides.
112
What is an alkali?
A soluable base.
113
What do acids produce in aquaeous solutions?
H+ ions
114
What do alkali's produce in aquaeous solutions?
OH- ions
115
What happens ina neutralization reaction?
H+ from acid and OH- from base react to form H2O, the remaining form salt.
116
the most common universal indicator is....
full-range.
## Footnote
there are solution and paper versions, full range is the most common(in liquid form)
117
Is universal indicator accurate?
No, a more useful indicator for pH is pH probe/pH meter.
118
pH is a measure of....
how many H+ ions are present.
119
2 soluable carbonates(alkaline bases)
Potsssium carbonate and Sodium carbonate are 2 water soluable carbonates. As carbonates are also bases, the fact they're soluable makes them alkalines.
120
Steps to carry out titration
- Use the pipette and pipette filler and place exactly 25 cm3 sodium hydroxide solution into the conical flask
- Place the conical flask on a white tile so the tip of the burette is inside the flask
- Add a few drops of a suitable indicator to the solution in the conical flask
- Perform a rough titration by taking the burette reading and running in the solution in 1 – 3 cm3 portions, while swirling the flask vigorously
- Quickly close the tap when the end-point is reached (sharp colour change) and record the volume, placing your eye level with the meniscus
- Now repeat the titration with a fresh batch of sodium hydroxide
- As the rough end-point volume is approached, add the solution from the burette one drop at a time until the indicator just changes colour
- Record the volume to the nearest 0.05 cm3
- Repeat until you achieve two concordant results (two results that are within 0.1 cm3 of each other) to increase accuracy
121
Which carbonate salts are soluable?
Sodium, potassium and Ammonium carbonate are the only soluble carbonate salts.
## Footnote
The rest are insoluable.
122
Which sulphate salts are soluable?
All of them except;
- Barium sulphate
- Calcium sulphate
- Lead(II) sulphate
123
Which hydroxide salts are soluable?
Sodium, potassium, magnesium, and calcium hydroxide are soluble salts. the rest are insoluble.
124
Which phosphate salts are soluble?
- All group 1 metals
- Ammonium phosphate
## Footnote
the rest are insoluble
125
Name 4 salts which are ALWAYS soluble.
**- All** Sodium
**- All** Potassium
**- All** Ammonium
**- All** Nitrates
126
Which chloride salts are soluble?
All of them except Silver and lead chloride salts.
127
3 ways to make a soluble salt with an acid?
- Metal+ acid
- Metal oxide or metal hydroxide+acid
- metal carbonate+ acid
128
What is seen as Magnesium reacts with acids?
effervesence and fizzing.
129
Reaction of zinc with acids?
| a property of the reaction once compared to magnesium
Slower than magnesium as lower in the reactivity series
130
What's seend when copper(II) oxide reacts with dilute sulphuric acid?
The copper(II)oxide powder(black) makes a blue solution
131
name some soluble metal oxides(alkalis)
- all of group one
- calcium oxides
- ammonia oxide.
132
What's a change when sodium hydroxide reacts with an acid?
temperature change
133
What's seen when copper carbonate reacts with common acids?
Green Solution turns into blue/blue-green solution.
134
Method to form insoluble salts
- mixing 2 soluble salts in water(so the mixture has water, a soluble salt, and an insoluble salt)
- filter it
- wash the crytals
- dry them
## Footnote
is good for forming lead(II) and silver nitrates.
135
Defien preciptation reaction
two soluble soltuions form an insoluble one
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# this will form:
Lead Nitrate+Potassium sulphate ---> Lead sulphate + Potassium Nitrate
an insoluble salt lead sulphate, and soluble potassium nitrate from 2 soluble salt solutions.
137
Method B of forming a soluble salt
| (involves titration)
- Use a pipette to measure the alkali into a conical flask and add a few drops of indicator (phenolphthalein or methyl orange)
- Add the acid into the burette and note the starting volume
- Add the acid very slowly from the burette to the conical flask until the indicator changes to appropriate colour
- Note and record the final volume of acid in burette and calculate the volume of acid added (starting volume of acid - final volume of acid)
- Add this same volume of acid into the same volume of alkali without the indicator
- Heat to partially evaporate, leaving a saturated solution
- Leave to crystallise decant excess solution and allow crystals to dry
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method A of forming soluble salt
- Heat acid and add insoluble metal (or oxide or carbonate) in excess(so excess acid does not become concentrated once heated
- filter products
- crystalization
139
# What has formed?
CuO (s) + H2SO4 (aq) ⟶ CuSO4 (s) + H2O (l)
- Neutralization as salt and water
- soluble salt copper sulphate
140
BAWS
base+acid--->water+salt
141
CAWCS
Carbonate+acid--->water+carbon dioxide+salt
142
MASH
metal+acid--->salt+hydrogen
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equiptment to prepare hydrated salt
| (named salt being copper(II)sulphate)
- 1.0 mol / dm3 dilute sulfuric acid
- Copper(II) oxide
- Spatula & glass rod
- Measuring cylinder & 100 cm3 beaker
- Bunsen burner
- Tripod, gauze & heatproof mat
- Filter funnel & paper, conical flask
- Evaporating basin and dish.
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