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N5 Chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

Whats a standard solution

A

Its a solution with an accurately known concentration.

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2
Q

What does the pH scale measure

A

The pH scale measures the acidity or alkalinity of solution. A pH less than 7 is acidic. Alkalis dissolve in water to give a pH greater than 7. A pH equal to 7 indicated a neutral solution.

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3
Q

Name 3 acids and their formula

A

Hydrochloric acid-HCl
Sulfuric acid-H2SO4
Nitric acid-HNO3

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4
Q

Name 3 alkalis and their formula

A

Sodium hydroxide-NaOH
Calcium Hydroxide-Ca(OH)2
Lithium hydroxide-LiOH

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5
Q

What happens when an alkali is diluted

A

The concentration of OH- ions is decreased and the pH decreases towards 7.

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6
Q

What happens in water and neutral solutions

A

The concentration of hydrogen ions id equal to the con of hydroxide ions

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7
Q

Whats neutralisation

A

This is the reaction of an acid with a base that results in the pH moving towards 7.

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8
Q

2 example equations of neutralisation

A

Acid + alkali —-> salt + water
Acid + metal oxide —-> salt + water

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9
Q

How do you name a salt

A

The metal ion from the alkali replaces the hydrogen ion from the acid (alkali to front, acid to back)

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10
Q

What is the salt name ending for hydrochloric, sulfuric and nitric acid

A

Chloride
Sulfate
Nitrate

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11
Q

What happens during neutralisation

A

The H+ ion from the acid joins with the OH- ion from the alkali

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12
Q

What do non-metals form

A

Negative ions

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13
Q

What do metals form

A

Positive ions

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14
Q

What equipment do you need to make a standard solution

A

Volumetric flask, Beaker, Wash bottle, 3 d.p balance, stirring rod, spatula, pipette dropper, deionised water, weighing boat, funnel

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15
Q

Whats the method to making a standard solution

A

•first calculate mass of solute needed
•Then weigh it into weighing boat using 3 d.p balance
•Then transfer into beaker ensure all solute is transferred by rinsing the weighing boat with distilled water
•Ensure all of the solute has been dissolved then swirl the solution
•Once dissolved transfer into volumetric flask DONT SPILL
•Then rinse to ensure none of the original solution is left do this 2-3 times
• Once rinsed place stopper
•gently shake
•Then fill up volumetric flask with distilled water until the bottom of the meniscus is touching the line

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16
Q

What factors affect the reaction rate

A

•Temperature
•Concentration
•Particle size
•Use of catalyst

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17
Q

Whats the collision theory

A

For a reaction to occur, the particles that are reacting must collide with each other. Only some collisions take place cause a chemical reaction to happen. These are called successful collisions. The greater the number of successful collisions, the faster the rate of reaction.

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18
Q

What are the three different ways to monitor the rate of reaction

A

•3dp balance
•Gas syringe
•Measuring cylinder

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19
Q

How do you calculate average rate of reaction

A

Average rate= Change in quantity/change in time

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20
Q

Whats an independent variable

A

The variable that is being changed during the experiment.

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21
Q

Whats an dependent variable

A

The variable being tested/measured during the experiment.

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22
Q

Whats an electrons mass, charge and location

A

Mass:Approx 0
Charge:-1
Location:Energy level

23
Q

Whats a protons mass, charge and location

A

Mass:1 amu
Charge:+1
Location:Nucleus

24
Q

Whats a Neutrons mass, charge and location

A

Mass:1 amu
Charge:0
Location:Nucleus

25
Q

Whats an atoms overall charge

A

Every atom has no overall charge

26
Q

What are horizontal and vertical lines called on the periodic table

A

Horizontal-Periods
Vertical-Groups

27
Q

What are four major signs of a chemical reaction

A

•colour change
•energy produced
•Gas released
•New substance formed

28
Q

What are the properties of alkali metals (group 1)

A

They are soft metals with low density that react rapidly with water producing an alkaline solution and hydrogen gas. The metals become more reactive as you go down the group

29
Q

What are the properties of the alkaline earth metals (group 2)

A

They are slightly less reactive, harder and denser than group 1

30
Q

What are the properties of the halogens (group 7)

A

Fluorine and chlorine are gases. Bromine is one of only two liquid elements. Iodine is solid. They exist as diatomic molecules-they have two atoms in each molecule. As you go down the group the halogens become less reactive.

31
Q

What are the properties of the noble gases (group 0)

A

They are very unreactive and exist as individual atoms

32
Q

What are the properties of the transition metals

A

They are found between group 2 and 3. Examples are iron, copper and gold. They are generally quite dense and many form brightly coloured compounds.

33
Q

What does the atomic number tell us

A

How many protons that element has.

34
Q

Whats the maximum amount of electrons the first energy level can hold

A

Two electrons

35
Q

Whats the maximum amount of electrons the other energy shells can hold

A

Maximum of 8 electrons

36
Q

Whats the mass number

A

The mass number tells us the number of protons and neutrons in an atom

37
Q

Whats an isotope

A

An isotope are atoms with the same atomic number but a different mass number

38
Q

How to atoms form a stable electron arrangement

A

Atoms can either lose, gain or share electrons

39
Q

Whats a covalent bond

A

A covalent bond is a shared pair of electrons between atoms of two non-metal elements.

40
Q

What are the 7 diatomic elements

A

Iodine, Bromine, Chlorine, Fluorine, Oxygen, Nitrogen, Hydrogen

41
Q

What structure does a diamond have

A

Tetrahedral structure

42
Q

What are ionic bonds formed between

A

Ionic bonds formed between a metal and a non-metal

43
Q

What structure do Ionic compounds form

A

Lattice Structure

44
Q

What happens to the outer electrons in metallic bonding

A

They become delocalised (free to move)

45
Q

What are the properties of Ionic lattice

A

Ionic lattice have high boiling and melting points, they are solid at room temperature and they only conduct electricity when molten or in solution.

46
Q

What are the properties of covalent network

A

In covalent network the boiling and melting points are very high, they are solid at room temperature and they never conduct electricity except graphite

47
Q

What are the properties of Discrete Covalent molecules

A

Discrete covalent molecules have low melting or boiling points, they are liquid or gas at room temperature and they never conduct electricity

48
Q

What are the properties of Metallic

A

Metallic generally have high melting and boiling points, they are solid at room temperature (except mercury which is liquid) they conduct electricity

49
Q

Whats electrolysis

A

Electrolysis is the breaking up of an ionic solution using electricity

50
Q

What are alkalis

A

They are soluble bases. An alkaline solution can be formed when a metal oxide is dissolved in water

51
Q

How is an acidic solution formed

A

They are formed when a non-metal is dissolved in water

52
Q

Why do we carry out titration experiments

A

Titration experiments can be carried out to accurately measure the volume of substances that react in chemical reactions. This technique is commonly used in neutralisation reactions and can also be used to calculate an unknown concentration

53
Q

How do you carry out a titration experiment

A
  1. If the sample is solid its weighed using an accurate balance, this is then dissolved to make up a known volume of solution
  2. A pipette is used to measure accurately a volume of this solution. A safety pipette filler is used to draw solution into the pipette. This is emptied into a conical flask.
  3. A few drops of indicator may be added to the conical flask. This will show a change of colour when the titration is complete.
  4. A second chemical is places in the burette. The other solution is of a chemical that will react with the synthesised chemical sample in the conical flask. Often the solution in the burette is an acid acid of a precise known concentration
  5. The solution from the burette is run into the conical flask. The solution is added one drop at a time, with swirling to mix the solutions as the end-point is approached. Eventually, a colour change shows that the correct amount has been added to react completely with the synthesised chemical in the sample.
  6. The volume of solution added from the burette is noted. The titration results can then be used to calculate the amount of the synthesised chemical in the sample, and therefore find its purity.
54
Q

What equipment do you use for titration

A

Burette, Conical flask, Pipette filler and Pipette

N5 Chemistry (3 decks)

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