Ark Elvin Academy Year 9 Science Study Pack Spring assessment 2018

20 Pages·2017·0.97 MB·English

by  Ms Flanagan

Ark Elvin Academy
Year 9 Science Study Pack
Spring assessment 2018

Name __________________

What I am going to be assessed on?
You will be assessed on everything that you have been taught so far in
Year 9 in both the autumn (before Christmas) and spring term (January
and February).
To help you revise the key content use your kerboodle login and access the
online textbooks.

Content overview

Cumulative content – you will also be examined on

content that you were taught in Y9 Term 1. ‘Cumulative

content’ will make up 40% of the Spring 1 examinations.
Year 9 Spring 1 (Jan/Feb): what are we learning and what will we be assessed on in our
Spring examinations?
Biology Topic – Digestion
Key concepts: Cell organization, enzymes, investigating enzymatic
reactions, enzymes and digestion, factors affecting enzymes in
digestion, food tests, catalysts
Topic – Respiration
Key concepts: Aerobic respiration, Anaerobic respiration, Exercise and
respiration, metabolism
Chemistry Topic – The Periodic table
Key concepts: Development of the periodic table, The modern Periodic
Table, metals and non-metals, Group 1 elements (alkali metals), Group 7
elements (halogens), Group 0 elements (noble gases)
Physics Topic – Energy transfer by heating
Key concepts: Conduction, convection, insulation, infra-red radiation,
specific heat capacity, reducing energy loss in houses

How many exams will I have?
3 x 30 minutes papers
1 Biology exam, 1 Chemistry exam and 1 Physics exam
Chemistry
Periodic table

Key knowledge

The periodic table – history
 Three key Scientists contributed to the periodic table in the 1800s: Dalton, Newland and
Mendeleev
Dalton Newland Mendeleev
Ordered elements by relative Ordered elements by relative Ordered elements by relative
atomic mass atomic mass. atomic mass.
Newland found that each Mendeleev switched the order to
element was similar to the fit the preoprties of elements e.g.
element eight places further on. Te and I. iodine has a smaller
For example, starting at Li, Be is relative atomic mass than
the second element, B is the third tellerium but had similar
and Na is the eighth element. properties to the group after
There were problems e.g. iron (a Tellerium.
metal) was in the same group as Gaps were left to make sure
sulphur and oxygen elements of the same properties
were in the same group.
Gaps indicated the existence of
undiscovered elements and
allowed Mendellev to predict
what the properties might be.

 Scientists did not know about atomic strutcure (protons, neutrons and electrons) and
therefore, were unable to order elements by atomic number
 Why were Mendeleev’s ideas accepted?
1. Discovery of isotopes – isotopes of the same element have different atomic masses but the
same chemical properties so occupy the same position on the periodic table
2. Discovery of sub-atomic particles
3. Newly discovered elements fit Mendeleev’s predictions

The periodic table – modern
Intro
The periodic table has elements in order of their atomic number and organised according to properties.
The name of the periodic table originates as the elements are said to be arranged ‘periodically’ meaning that
there are repeating patterns.
We now know that the reason why elements in a group have similar properties is because they have the
same number of electrons in the outer shell.
Groups are the columns and periods are the rows.
Groups
 The group number tells you how many electrons are in the outer shell (number of valence
electrons)
 Elements in the same group have similar chemical properties and react in a similar way

Periods
 The period number tells us how many occupied shells (energy levels) there are; each new
period represents another full shell of electrons.

Metals
 Approximately 4/5 of the elements in the periodic table are metals
 Metals are situated on the left and centre of the periodic table
 Metals react to form cations (positively charged ions)
Properties
 Strong and malleable
 High conductivity (thermal and electrical)
o High melting and boiling points

Non metals
 Approximately 1/5 of the elements in the periodic table are non-metals
 Non-metals are situated on the right of the periodic table
 Non-metals react to form anions (negatively charged ions)

Group 7 - Halogens
Physical properties Electronic structure Chemical reactions Trends
Non-metals 7 valence electrons React with hydrogen to As the group descends:
Fluorine  yellow gas Gain 1 electron to form - form covalent
Chlorine  green gas 1 anions to form a full molecules e.g. hydrogen 1. The elements
Bromine  red-brown octet fluoride become less
liquid Exist as diatomic reactive
Iodine  dark grey covalent molecules e.g. Hydrogen + fluorine  2. Higher melting
solid Br2 hydrogen fluoride and boiling
H + F  2HF points
2 2

Reaction with metals to
Why are the group 7
form ionic compounds
elements less reactive at
e.g. sodium bromide
the bottom of the

group?
sodium + bromine 

sodium bromide
The size of the atom
2Na + Br  2NaBr
2
increases because there

are more electron shells
React during
The outer shell is
displacement reactions.
further away from the
A displacement reaction positive nucleus due to
is defined as A more increased shielding
reactive halogen can (increase no. of shells
displace a less reactive between the nucleus
halogen from an and valence shell), so
aqueous solution of its when an electron is
salt transferred to the
halogen the attraction is
e.g. chlorine + weaker than at the top
potassium iodide  of the group where the
potassium chloride + nuclear attraction is
iodine stronger due to less
Cl + 2KI  2KCl + I shielding
2 2

Group 1 – Alkali metals

Physical properties Electronic structure Chemical reactions Trends
Metals 1 valence electron React with water to As the group descends:
Soft Lose an electron to form form metal hydroxides:
Low density +1 cation to form a full Group 1 metals react 1. The elements
octet vigorously n water to become more
form metal hydroxides reactive
which turn the water 2. Lower melting
blue when universal and boiling
indicator is present as points
hydroxides are alkaline.

During this reaction
Why are the group 71
hydrogen gas. The
elements more reactive
presence of hydrogen
at the bottom of the
can be test form using a
group?
lit splint, a positive test

will form a squeaky pop.
The size of the atom

increases because there
Sodium + water 
are more electron
sodium hydroxide +
shells.
hydrogen
The outer shell is
2Na + 2H O  2NaOH
2
further away from the
+ H
2
positive nucleus due to

increased shielding
(increase no. of shells
Reaction with chlorine between the nucleus
to form ionic and valence shell).
compounds When a group 1 atom
e.g. sodium chloride reacts it will form a +1
sodium + chlorine  ion and therefore, needs
sodium chloride to lose an electron. As
2Na + Cl  2NaCl the group descends the
2
nuclear attraction
Reaction with oxygen to between the positively
form ionic compounds charged nuclear and
e.g. sodium oxide valence electron
sodium + oxygen  decreases and can be
sodium oxide lost more readily.
4Na + O  2Na O
2 2

Group 0 – Noble gases

Physical properties Electronic structure Trends
Non-metals He – 2 electrons in the As the group descends:
Inert outer shell which is a
Colourless gases full first energy level 1. The boiling point of the noble gases increase
Non-flammable All other noble gases

have 8 electrons in the
Why are the boiling points of the noble gases higher
valence shell and
at the bottom of the group?
therefore have a full
The atomic number of each atom increases as the
outer shell.
group descends, meaning there are a greater
Outer shell is
number of electrons in each atom leading to greater
energetically stable and
intermolecular forces between atoms which require
therefore, they are inert
a greater amount of energy to overcome.
(do not need to
lose/gain electrons)

Monoatomic – travel
around as single atoms.
Key questions

The periodic table – history

1. Name three scientists who contributed to the periodic table
2. How were the elements in the periodic table first organised?
3. Which scientist improved the periodic table by leaving gaps for elements he hadn’t thought had been
discovered?
4. Why did people begin to accept this structure of the periodic table?
5. Evaluate whether hydrogen has been put in the correct place on an early version of the periodic table
below. Justify your answer.

The periodic table – modern
1. What fraction of the periodic table is made up of metals
2. Define the term period
3. Define the term group
4. In what order are elements in the periodic table organised? E.g. why does carbon come before nitrogen?
5. What is similar about the electronic structure of the elements of group 1 (Li, Na, K etc.)?
6. Name 2 elements in the periodic table that react in a similar way and explain the reason for this.
7. If an element is in group 1, period 3 what does is tell you about the element’s electronic structure?
8. Do metals form positive or negative ions? Why?
9. Do non-metals form positive or negative ions? Why?
10. Complete the table to show the ion formed from each atom.
Element name Number of electrons Will it lose or gain Charge
Group
and symbol in outer shell electrons? How many? on ion
Lithium, Li 1 1 Will lose one Li+
Beryllium, Be Be2+
Oxygen, ____ 6 6 Gain two O2-
_________, N
Boron, B
Fluorine,

_______
P3-
Rb+
11. Use the periodic table to name the elements represented by the electronic structures below

Group 7
1. What is another name for the group 7 elements?
2. How many electrons do group 7 elements have on their outer shell?
3. Write the formula for a molecule of chlorine.
4. Which group 7 element
a) Has the highest melting point?
b) Has the lowest boiling point?
5. Why is fluorine the most reactive halogen?
6. Would a displacement reaction take place if chlorine gas was reacted with potassium bromide? Explain
your answer.
7. Write a word and symbol equation for the reaction between bromine and lithium iodide.
8. In the reaction above, identify the two elements and the two compounds.
9. What kind of substance is potassium fluoride?
10. Explain why potassium fluoride has a higher melting point than fluorine.
11. Explain why iodine is less reactive than bromine.

Group 1
1. State the other name for the group 1 elements.
2. How many electrons do group 1 elements have on their outer shell?
3. Describe and explain the trend in the reactivity of group 1 metals as you descend group 1?
4. Which group 1 element is the least reactive? Why?
5. Complete the table to describe the reactions of the first 3 group 1 elements with oxygen, chlorine and
water.
Group 1 Reaction with Reaction with Reaction with
Metal oxygen chlorine water
Lithium

Sodium

Potassiu
m

6. Write a word and symbol equation for the reaction between potassium and:
a. Oxygen
b. Chlorine
c. Water
7. Explain what the different state symbols in your equations stand for
8. A student drops 2g of lithium into 150g of water in a beaker. Explain why the mass of the beaker weighs
less than 152g at the end.
9. This question is about the reaction below:
2Li(s) + Cl (g)  2LiCl(s)
2
a. Explain why chlorine is a gas at room temperature
b. Under what conditions will lithium chloride conduct electricity?
c. Why does lithium conduct electricity?

Group 0
1. What is another name for the group 0 elements?
2. How is the electron configuration of group 0 elements similar?
3. How does the electron configuration of group 0 elements affect their reactivity?
4. Does neon or krypton have a higher boiling point? What is the trend as you go down the group?
5. Why are the group 0 elements described as monoatomic?
Biology
Respiration

Key knowledge
The importance of respiration
Respiration is an examples of an exothermic reaction. An exothermic reaction is deifned as a reaction that
releases eergy; it relseases energy from glucose molecules for use in the body.
Aerobic respiration happens all the time in the cells of animals and plants. Most of the reactions involved
happen inside mitochondria, tiny organelles inside the cytoplasm of the cell. The reactions are controlled by
enzymes.
What do organisms need energy from respiration for?
1. Chemical reactions to build larger molecules
2. Movement
3. Maintain body temperature
Aerobic respiration
Aerobic respiration is the form of respiration which uses oxygen. It can be summarised by this equation:
Glucose + oxygen → carbon dioxide + water (+ energy)
Energy is shown in brackets because it is not a substance. Notice that:
 Glucose and oxygen are used up
 Carbon dioxide and water are produced as waste products
Aerobic respiration happens all the time in the cells of animals and plants. Most of the reactions involved
happen inside mitochondria, tiny organelles inside the cytoplasm of the cell. The reactions are controlled by
enzymes.
Anaerobic respiration
 Glucose is not completely broken down due to a lack of oxygen
 Anaerobic respiration transfers less energy
 Anaerobic respiration happens in plants, yeast and animals

Human anaerobic respiration
Glucose  lactic acid

Anaerobic respiration in plants and yeast
Glucose  ethanol + carbon dioxide

 Anaerobic respiration in yeast is called fermentation. Fermentation is
important in the manufacturing of break and alcoholic drinks (beer and
wine)

Exercise and respiration
 During exercise, the body demands more enegry so the rate of respiration increases. The muscles require
energy for the protein fibres to contract.
 The heart rate, breathing rate and breath volume all increase to supply the muscles with more oxygen and
glucose for the increase in aerobic respiration.