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AQA Chemistry GCSE Unit 4.1 Atomic Structure and the Periodic Table – Foundation 1
Draw and label an atom. Include labels for the following: a What are the symbols for the following elements. d Complete and balance the following equations. g Separating Mixtures k
neutron, proton, electron. What are the following separation techniques?
Element Symbol Mg + O MgO
2
oxygen
Be + S BeS
lithium
Be + F
sodium 2
K + Cl
potassium 2
helium
D
True or false? carbon h
1. The radius of an atom is 0.1nm. Mixtures
2. Most of the mass is in the shell of the atom. magnesium Write the definition of a mixture. Give two examples.
Fill in the table to show the charges and mass of the b Complete the following diagram for sodium, include the e
components of an atom. atomic number and the atomic mass number.
Name Charge Relative Mass
proton
neutron Na F D
Name the compounds and the elements they contain. i
electron What separation technique would you use to separate out
What is the overall charge of an atom? different inks in pens?
positive What is the mass number? NaCl - sodium chloride, sodium and chlorine
negative MgO - C
no charge How do you calculate neutron number? MgS -
How can salt be collected using the process of crystallisation?
A compound is 2 or more e , chemically c FeS -
j . Isotopes are elements with a different number of f
Which of the following are compounds? n but the same number of p , What is the ratio of the elements in the following j
e.g. carbon 12 and carbon 14. compounds? Sand and water can be separated by using a process called
Put a ring round them. F
oxygen, salt water, magnesium oxide, sodium chloride, How can you use isotopes to calculate the relative atomic
mass? Write down the equation. e.g. CaO = 1:1 NaCl = Describe in 4 steps how to collect salt from rock salt.
nitrogen
Relative atomic = sum of ( ) MgCl = lithium fluoride = 1.
Why have you circled the ones you have? mass (Ar) 2
2.
K 0 = sodium hydroxide = 3.
2
4.
AQA Chemistry GCSE Unit 4.1 Atomic Structure and the Periodic Table – Foundation 2
Complete the electronic structure diagrams for: a List 3 halogens d Complete the following dot and cross diagrams for: g Describe the plum pudding model of the atom. j
oxygen c , f , i , NaCl Draw a diagram.
How many electrons do they have in their outer shell?
O Circle the correct answer.
a) 1 b) 7 c) 8
magnesium Describe how the reactivity changes as you go down the group.
Keywords: reactive, nucleus, distance, less
Mg
MgO
Write balanced symbol equations for the following reactions: Why did scientists believe this model?
What are the following gases? b
A n, N n, X n, R n bromine + potassium iodide
Describe what the alpha scattering experiment showed k
Describe why the noble gases are so unreactive. chlorine + sodium iodide scientists.
Keywords: full, electrons, shell.
Keywords: alpha, gold, positive, gold, scattered particles
fluorine + potassium chloride
Underline the properties of metals and circle the e Complete word equations for the following reactions: h
The boiling points of the noble gases increase/decrease as
you go down the group. (delete the wrong answer). properties of non-metals:
Can you explain your answer? e.g. sodium + chlorine sodium chloride
strong, low density, malleable, dull, good conductors
of heat and electricity, high melting and boiling point, lithium + iodine
brittle, not good conductors of electricity.
potassium + bromine
Describe what happens to the reactivity of the alkali c James Chadwick discovered the… f
metals as you go down the group. (underline the correct answer) How are the groups arranged in the periodic table? i Niels Bohr discovered that l
proton
Why?
neutron How can you tell that the alkali metals are very reactive?
Hint: Think about the number of electrons in the outer shell. Why did Mendeleev leave gaps in the periodic table?
electron
Complete the word and symbol equation for sodium
reacting with water: How can you tell the noble gases are unreactive?
sodium + water sodium hydroxide + What happened to some of the gaps he left?
Na + NaOH +
AQA Chemistry GCSE Unit 4.1 Atomic Structure and the Periodic Table – Foundation Answers 1
Draw and label an atom. Include labels for the following: a What are the symbols for the following elements. d Complete and balance the following equations. g Separating Mixtures k
neutron, proton, electron. What are the following separation techniques?
Element Symbol Mg + O MgO
2
oxygen
Be + S BeS
lithium
Be + F BeF
sodium 2 2
electrons
K + Cl 2KCl
neutrons potassium 2
protons
helium
True or false? Distillation
1. The radius of an atom is 0.1nm. True carbon h
2. Most of the mass is in the shell of the atom. False, most Mixtures
of the mass is in the centre magnesium Write the definition of a mixture. Give two examples.
Two or more elements together, not chemically joined and
Fill in the table to show the charges and mass of the b Complete the following diagram for sodium, include the e
components of an atom. atomic number and the atomic mass number. can be easily separated.
Name Charge Relative Mass Salt water, sand and water
proton 23 mass number
neutron Na Fractional distillation
Name the compounds and the elements they contain. i
electron 11 atomic number What separation technique would you use to separate out
What is the overall charge of an atom? different inks in pens?
No charge What is the mass number? NaCl - sodium chloride, sodium and chlorine
Total number of protons and neutrons. MgO - magnesium oxide, magnesium and oxygen Chromatography
How do you calculate neutron number? MgS - magnesium sulfide, magnesium and sulfur
Atomic mass – proton number How can salt be collected using the process of crystallisation?
A compound is 2 or more elements, chemically joined. c FeS - iron sufide, iron and sulfur By heating up a mixture of salt and water, the water will
Isotopes are elements with a different number of f evaporate and leave the salt in the bowl.
Which of the following are compounds? neutrons but the same number of protons, e.g. carbon j
Put a ring round them. 12 and carbon 14. What is the ratio of the elements in the following Sand and water can be separated by using a process called
compounds? filtration.
oxygen, salt water, magnesium oxide, sodium chloride, How can you use isotopes to calculate the relative atomic
nitrogen mass? Write down the equation. e.g. CaO = 1:1 NaCl = 1:1 Describe in 4 steps how to collect salt from rock salt.
Why have you circled the ones you have? 1. Grind the mixture;
sum of (isotope abundance x isotope mass number)
Ar = MgCl = 1:2 lithium fluoride = 1:1 2. Add water and stir;
They have 2 or more elements in the word equation. sum of abundances of all the isotopes. 2
3. Filter the mixture;
K 0 = 2:1 sodium hydroxide = 1:1:1 4. Evaporate the salt water and salt is left over.
2
AQA Chemistry GCSE Unit 4.1 Atomic Structure and the Periodic Table – Foundation Answers 2
Complete the electronic structure diagrams for: a List 3 halogens d Complete the following dot and cross diagrams for: g Describe the plum pudding model of the atom. j
oxygen chlorine, fluorine, iodine, astatine NaCl Draw a diagram.
How many electrons do they have in their outer shell? A sphere of positive
7 electrons charge with electrons
dotted about; looking like a plum
Describe how the reactivity changes as you go down the pudding.
group.
They become less reactive, the atom becomes larger
magnesium because there are more electron shells, further from the
nucleus so the pull of the nucleus is less. So the electron
is less likely to be gained as there is less of a positive pull.
Write balanced symbol equations for the following reactions: MgO
bromine + potassium iodide Why did scientists believe this model?
Br + 2KI 2KBr + I Lack of experimental evidence.
2 2
What are the following gases? b chlorine + sodium iodide k
Cl + 2NaI 2NaCl + I Describe what the alpha scattering experiment showed
argon, neon, xenon, radon 2 2
scientists.
Describe why the noble gases are so unreactive. fluorine + potassium chloride
F + KCl 2KF + Cl Most alpha particles go straight through, some are
Their outer shell is full of electrons. 2 2 scattered, some rebound off the gold foil.
This shows that the nucleus of an atom has a very small
The boiling points of the noble gases increase as you go Underline the properties of metals and circle the e Complete word equations for the following reactions: h radius. Most of the mass is concentrated in the nucleus.
down the group. properties of non-metals:
This is because there are more forces to bond the atoms sodium + chlorine s odium chloride
together, therefore more energy is required to break the strong, low density, malleable, dull, good conductors
bonds. of heat and electricity, high melting and boiling point, lithium + iodine lithium iodide
c brittle, not good conductors of electricity.
Describe what happens to the reactivity of the alkali potassium + bromine potassium bromide
metals as you go down the group. James Chadwick discovered the… f
It increases (underline the correct answer) i l
How are the groups arranged in the periodic table? Niels Bohr discovered that
Why? proton According to their properties. electrons orbit the nucleus in shells.
The number of electrons increases. They are further away
from the nucleus. There is less pull on the outer electrons neutron Why did Mendeleev leave gaps in the periodic table?
so the atom is more likely to loose an electron. How can you tell that the alkali metals are very reactive? He knew that the elements existed but they hadn’t been
electron According to their properties. found, based on their mass.
Complete the word and symbol equation for sodium
reacting with water: What happened to some of the gaps he left?
sodium + water sodium hydroxide + hydrogen How can you tell the noble gases are unreactive? They have been filled. Scientists have found some of the
2Na + 2H O 2NaOH + H Full shell of outer electrons. elements.
2 2
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