Embed Size (px)
Citation preview
1.1 Simple model, symbols, RAM, charge, isotopes - Standard demand – Questions
Q1.There are eight elements in the second row (lithium to neon) of the periodic table.
(a) Figure 1 shows an atom with two energy levels (shells).
(i) Complete Figure 1 to show the electronic structure of a boron atom.(1)
(ii) What does the central part labelled Z represent in Figure 1?
____________________________________(1)
(iii) Name the sub-atomic particles in part Z of a boron atom.
Give the relative charges of these sub-atomic particles.
______________________________________________________________
______________________________________________________________
______________________________________________________________(3)
(b) The electronic structure of a neon atom shown in Figure 2 is not correct.
Page 1 of 33
Explain what is wrong with the electronic structure shown in Figure 2.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(Total 8 marks)
Q2.This question is about fluorine.
(a) Figure 1 shows the arrangement of electrons in a fluorine atom.
(i) In which group of the periodic table is fluorine?
Group _______________________________(1)
(ii) Complete the table below to show the particles in an atom and their relative masses.
Name of particle Relative mass
Proton
Neutron 1
Very small
(2)
(iii) Use the correct answer from the box to complete the sentence.
alkalis alloys isotopes
Page 2 of 33
Atoms of fluorine with different numbers of neutrons are
called ________________ .(1)
(b) Sodium reacts with fluorine to produce sodium fluoride.
(i) Complete the word equation for this reaction.
sodium + ___________________ → ____________________(1)
(ii) Complete the sentence.
Substances in which atoms of two or more different elements are chemically
combined are called _____________________ .(1)
(iii) The relative formula mass (Mr) of sodium fluoride is 42.
Use the correct answer from the box to complete the sentence.
ion mole molecule
The relative formula mass (Mr), in grams, of sodium fluoride is one
_______________ of the substance.(1)
(iv) Figure 2 shows what happens to the electrons in the outer shells when a sodium atom reacts with a fluorine atom.
The dots (•) and crosses (×) represent electrons.
Use Figure 2 to help you answer this question.
Describe, as fully as you can, what happens when sodium reacts with fluorine to produce sodium fluoride.
______________________________________________________________
______________________________________________________________
______________________________________________________________
Page 3 of 33
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________(4)
(v) Sodium fluoride is an ionic substance.
What are two properties of ionic substances?
Tick (✔) two boxes.
Dissolve in water
Gas at room temperature
High melting point
Low boiling point
(2)(Total 13 marks)
Q3.(a) The formula for ammonia is NH3. What does the formula tell you about each
molecule of ammonia?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(b) Ammonia is used to make nitric acid (HNO3). Calculate the formula mass (Mr) for nitric acid. (Show your working).
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(Total 6 marks)
Page 4 of 33
Q4.This question is about atomic structure and elements.
(a) Complete the sentences.
(i) The atomic number of an atom is the number of _______________________(1)
(ii) The mass number of an atom is the number of ________________________
______________________________________________________________(1)
(b) Explain why an atom has no overall charge.
Use the relative electrical charges of sub-atomic particles in your explanation.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(c) Explain why fluorine and chlorine are in the same group of the periodic table.
Give the electronic structures of fluorine and chlorine in your explanation.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(d) The diagram shows the electronic structure of an atom of a non-metal.
What is the chemical symbol of this non-metal?
Page 5 of 33
Tick ( ) one box.
Ar
O
S
Si
(1)
(e) When elements react, their atoms join with other atoms to form compounds.
Complete the sentences.
(i) Compounds formed when non-metals react with metals consist of
particles called _________________________ .(1)
(ii) Compounds formed from only non-metals consist of
particles called ____________________ .(1)
(Total 9 marks)
Q5.This question is about atoms and isotopes.
(a) Atoms contain protons, neutrons and electrons.
A lithium atom has the symbol
Explain, in terms of sub-atomic particles, why the mass number of this lithium atom is 7.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
Page 6 of 33
(b) Amounts of substances can be described in different ways.
Complete the sentences.
One mole of a substance is the relative formula mass in
___________________________________________________________________
The relative atomic mass of an element compares the mass of an atom of an element with the mass of an atom of
___________________________________________________________________(2)
(c) Two isotopes of oxygen are and
Describe the similarities and differences between the isotopes and
You should refer to the numbers of sub-atomic particles in each isotope.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(Total 8 marks)
Q6.The Sun produces helium atoms from hydrogen atoms by nuclear fusion reactions.
Hydrogen Helium
(a) Describe the differences in the atomic structures of a hydrogen atom and a helium atom.
___________________________________________________________________
___________________________________________________________________
Page 7 of 33
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(b) The Sun consists of 73% hydrogen and 25% helium.The rest is other elements.One of the other elements in the Sun is neon.
Use the Chemistry Data Sheet to help you to answer these questions.
(i) Complete the diagram to show the electronic structure of a neon atom.
(1)
(ii) Why is neon in the same group of the periodic table as helium?
______________________________________________________________
______________________________________________________________
______________________________________________________________(1)
(Total 5 marks)
Q7.Aluminium has many uses.
(a) An aluminium atom has 13 electrons.
(i) Draw the electronic structure of an aluminium atom.
Page 8 of 33
(1)
(ii) Name the two sub-atomic particles in the nucleus of an aluminium atom.
_____________________________ and _____________________________(1)
(iii) Why is there no overall electrical charge on an aluminium atom?
______________________________________________________________
______________________________________________________________(1)
(b) Rail tracks are made from steel.
Molten iron is used to weld rail tracks.
The reaction of aluminium with iron oxide is used to produce molten iron.
(i) Balance the chemical equation for the reaction.
(1)
(ii) Why does aluminium react with iron oxide?
______________________________________________________________
______________________________________________________________(1)
(Total 5 marks)
Q8. The diagrams show the electronic structure of four different atoms.
Page 9 of 33
Use the Chemistry Data Sheet to help you to answer these questions.
(a) Name the two sub-atomic particles in the nucleus of an atom.
___________________________________________________________________(1)
(b) Why is there no overall electrical charge on each atom?
___________________________________________________________________
___________________________________________________________________(1)
(c) Why is Atom A unreactive?
___________________________________________________________________(1)
(d) Which two of these atoms have similar chemical properties?Give a reason for your answer.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(Total 5 marks)
Q9.Calamine lotion is used to treat itching. The main ingredients are two metal oxides.
Page 10 of 33
(a) One of the metal oxides has a relative formula mass (Mr) of 81.
The formula of this metal oxide is MO.(M is not the correct symbol for the metal.)
The relative atomic mass (Ar) of oxygen is 16.
(i) Calculate the relative atomic mass (Ar) of metal M.
______________________________________________________________
______________________________________________________________
______________________________________________________________
Relative atomic mass (Ar) = _____________(2)
(ii) Use your answer to part (a)(i) and the periodic table on the Data Sheet to name metal M.
The name of metal M is ___________________________________ .(1)
(b) The other metal oxide is iron(III) oxide.
This contains iron(III) ions (Fe3+) and oxide ions (O2-).
(i) Explain in terms of electrons how an iron atom (Fe) can change into an iron(III) ion (Fe3+).
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________(2)
(ii) The diagram below represents the electronic structure of an oxygen atom (O).
Page 11 of 33
Complete the diagram below to show the electronic structure of an oxide ion (O2-).
(1)
(Total 6 marks)
Q10.Lead compounds have been used for thousands of years as colours in paint.
Johannes Vermeer [Public domain], via Wikimedia Commons
(a) A sample of a red oxide used in paint was found to contain 6.21 g of lead and 0.64 g of oxygen.
Calculate the empirical (simplest) formula of this compound.
You must show all your working to gain full marks.
Relative atomic masses: O = 16; Pb = 207.
___________________________________________________________________
Page 12 of 33
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(4)
(b) A problem with lead compounds is that they slowly react with hydrogen sulfide in the air. This produces lead sulfide which is black.
(i) Hydrogen sulfide has the formula H2S. The bonding in a molecule of hydrogen sulfide can be represented as:
H–S–H
Complete the diagram below to show the arrangement of the outer electrons of the hydrogen and sulfur atoms in hydrogen sulfide.Use dots (●) and crosses (x) to represent the electrons.You need only show the outer shell electrons.(Atomic numbers: H = 1; S = 16.)
(1)
(ii) Hydrogen sulfide has a low boiling point.
Explain why.
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________(2)
(iii) Lead white is also used in paint. The white colour slowly darkens when lead
Page 13 of 33
sulfide is produced.
The painting can be restored with hydrogen peroxide. This converts the black lead sulfide into white lead sulfate.
Balance the equation for the reaction between lead sulfide and hydrogen peroxide (H2O2).
PbS(s) + ______H2O2(aq) → PbSO4(s) + 4H2O(l)
(1)(Total 8 marks)
Q11.(a) The table gives information about two isotopes of hydrogen, hydrogen-1 and
hydrogen-2.
Hydrogen-1 Hydrogen-2
Atomic number 1 1
Mass number 1 2
An atom of hydrogen-1 is represented as:
Show how an atom of hydrogen-2 is represented.
(1)
(b) (i) Calculate the relative formula mass (Mr) of water, H2O
Relative atomic masses: H = 1; O = 16.
______________________________________________________________
______________________________________________________________
Relative formula mass (Mr ) = ______________________(1)
(ii) Simple molecules like water have low boiling points.
Explain why, in terms of molecules.
______________________________________________________________
______________________________________________________________
Page 14 of 33
______________________________________________________________
______________________________________________________________(2)
(c) Molecules of heavy water contain two atoms of hydrogen-2 instead of two atoms of hydrogen-1.
Explain why a molecule of heavy water has more mass than a normal water molecule.You should refer to the particles in the nucleus of the two different hydrogen atoms in your answer.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(Total 6 marks)
Q12.Iron is an essential part of the human diet. Iron(II) sulfate is sometimes added to white bread flour to provide some of the iron in a person’s diet.
(a) The formula of iron(II) sulfate is FeSO4
Calculate the relative formula mass (Mr) of FeSO4
Relative atomic masses: O = 16; S = 32; Fe = 56.
___________________________________________________________________
___________________________________________________________________
The relative formula mass (Mr) = _______________(2)
Page 15 of 33
(b) What is the mass of one mole of iron(II) sulfate? Remember to give the unit.
_______________(1)
(c) What mass of iron(II) sulfate would be needed to provide 28 grams of iron?
Remember to give the unit.
_______________(1)
(Total 4 marks)
Q13.This question is about oxygen atoms. The periodic table on the Data Sheet may help you to answer this question.
(a) (i) Oxygen atoms have 8 electrons.
Complete the diagram to represent the arrangement of electrons in an oxygen atom.Use crosses (×) to represent the electrons.
(1)
(ii) Name the part of the oxygen atom that is labelled A on the diagram.
______________________________________________________________(1)
(b) Two isotopes of oxygen are oxygen-16 and oxygen-18.
16 18 O O
8 8
oxygen-16 oxygen-18
Explain, in terms of particles, how the nucleus of an oxygen-18 atom is different from the nucleus of an oxygen-16 atom.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Page 16 of 33
___________________________________________________________________(2)
(Total 4 marks)
Q14.(a) A chemist was asked to identify a nitrogen compound. The chemist carried out an
experiment to find the relative formula mass (Mr) of the compound.
The Mr of the compound was 44.
Relative atomic masses: N = 14, O = 16
Draw a ring around the formula of the compound.
NO NO2 N2O4 N2O(1)
(b) Potassium nitrate is another nitrogen compound. It is used in fertilisers. It has the formula KNO3.
The Mr of potassium nitrate is 101.
Calculate the percentage of nitrogen by mass in potassium nitrate.
Relative atomic mass: N = 14.
___________________________________________________________________
___________________________________________________________________
Percentage of nitrogen = _______________ %(2)
(Total 3 marks)
Q15.Toothpastes often contain fluoride ions to help protect teeth from attack by bacteria.
Some toothpastes contain tin(II) fluoride.
This compound has the formula SnF2 .
(a) Calculate the relative formula mass (Mr) of SnF2.
Page 17 of 33
Relative atomic masses: F = 19; Sn = 119
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Relative formula mass (Mr) = _____________________(2)
(b) Calculate the percentage by mass of fluorine in SnF2.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Percentage by mass of fluorine = _____________________ %(2)
(c) A tube of toothpaste contains 1.2 g of SnF2.
Calculate the mass of fluorine in this tube of toothpaste.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Mass of fluorine = _____________________ g(1)
(d) The diagram represents the electron arrangement of a fluorine atom.
Explain how a fluorine atom can change into a fluoride ion, F–.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Page 18 of 33
___________________________________________________________________(2)
(Total 7 marks)
Q16.Iron ore contains iron oxide.
(i) Calculate the relative formula mass of iron oxide, Fe2O3.
Relative atomic masses: O = 16; Fe = 56.
___________________________________________________________________
___________________________________________________________________
Answer = ________________________(2)
(ii) Calculate the percentage by mass of iron in iron oxide.
___________________________________________________________________
Percentage of iron = _____________________ %(2)
(iii) Calculate the mass of iron that could be extracted from 1000 kg of iron oxide.
Use your answer to part (c) (ii) to help you with this calculation.
___________________________________________________________________
Mass of iron = __________________________ kg(1)
(Total 5 marks)
Q17.Calcium carbonate tablets are used to treat people with calcium deficiency.
(a) Calculate the relative formula mass (Mr) of calcium carbonate.
Relative atomic masses: C = 12; O = 16; Ca = 40.
Page 19 of 33
___________________________________________________________________
___________________________________________________________________
Relative formula mass = _______________(2)
(b) Calculate the percentage of calcium in calcium carbonate, CaCO3.
___________________________________________________________________
___________________________________________________________________
Percentage of calcium = _____________ %(2)
(c) Calculate the mass of calcium in each tablet.
___________________________________________________________________
___________________________________________________________________
Mass of calcium = __________________ g(2)
(d) An unwanted side effect of this medicine is that it can cause the patient to have ‘wind’ (too much gas in the intestine).
The equation below represents the reaction between calcium carbonate and hydrochloric acid (the acid present in the stomach).
CaCO3 (s) + 2HCl (aq) →CaCl2 (aq) + H2O (l) + CO2 (g)
Suggest why the patient may suffer from ‘wind’.
___________________________________________________________________
___________________________________________________________________(1)
(Total 7 marks)
Q18. The chemical equation for the formation of iron is:
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)
Calculate the relative formula mass of iron oxide, Fe2O3.
Relative atomic masses: O 16; Fe 56.
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
Page 20 of 33
Relative formula mass Fe2O3 = ________________(Total 2 marks)
Q19. The diagrams show three isotopes of potassium.
(i) In what way does the atomic structure show you that they are all atoms?
___________________________________________________________________
___________________________________________________________________(1)
(ii) Explain why these three atoms are called isotopes of potassium.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(Total 4 marks)
Q20. Follow the steps to find the percentage of iron in iron oxide.
Relative atomic masses: O 16; Fe 56.
(i) Step 1
Calculate the relative formula mass of iron oxide, Fe2O3.
Page 21 of 33
___________________________________________________________________
___________________________________________________________________(1)
(ii) Step 2
Calculate the total relative mass of just the iron atoms in the formula, Fe2O3.
___________________________________________________________________(1)
(iii) Step 3
Calculate the percentage (%) of iron in the iron oxide, Fe2O3.
___________________________________________________________________
___________________________________________________________________
Percentage of iron _________________ %(1)
(Total 3 marks)
Q21.Silicon is an extremely important element. More than a million tonnes of silicon are produced each year. Silicon is made by reducing silicon oxide (sand) with carbon (coke).
(a) (i) Complete the diagram below to show the arrangement of electrons in an atom of silicon. The Data Sheet may help you with this question.
(2)
(ii) Which electrons in the silicon atom take part in chemical reactions with other atoms?
______________________________________________________________
______________________________________________________________(1)
(iii) What features of all the atoms of the elements in group 4 of the Periodic Table might give them similar chemical properties?
______________________________________________________________
______________________________________________________________
Page 22 of 33
(1)
(b) Silicon is difficult to classify as a metal or a non-metal because it has properties which resemble both. Some of the properties of silicon are listed below.
• Silicon is a shiny blue/grey solid.• Silicon is placed in Group 4 of the Periodic Table.• Silicon has a relative atomic mass of 28.• Silicon has a very high melting point (1410ºC).• Silicon has a very high boiling point (2355ºC).• Silicon conducts electricity.• Silicon oxide will neutralise alkalis.• Silicon forms compounds in which the silicon atoms are bonded to other atoms
by covalent bonds.
(i) Select two properties from the list above in which silicon resembles a metal.
1. ____________________________________________________________
2. ____________________________________________________________(2)
(ii) Select two properties from the list above in which silicon resembles a non-metal.
1. ____________________________________________________________
2. ____________________________________________________________(2)
(Total 8 marks)
Q22.There are millions of different substances that make up our world. All these substances are made from chemical elements.
(a) What is an element?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________ (1)
(b) Many substances are compounds. What is a compound?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
Page 23 of 33
(Total 3 marks)
Q23.Use these relative atomic masses: H = 1; O = 16; Ca = 40to calculate the relative formula mass (Mr ) of
quicklime CaO ___________________________________________________________
slaked lime Ca(OH)2______________________________________________________(Total 2 marks)
Q24.Use the Periodic Table of Elements on the Data Sheet to help you to answer this question.
(a) Describe, in as much detail as you can, the structure of a fluorine atom.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(b) Complete the diagram to show the electronic structure of a magnesium atom.
(1)
(Total 4 marks)
Q25.Ammonium chloride, NH4Cl, is made up of nitrogen, hydrogen and chlorine atoms.
(i) Complete the table to show the number of atoms of each element present in NH4Cl.
Element Number of atoms in
Page 24 of 33
NH4Cl
nitrogen 1
hydrogen
chlorine
(1)
(ii) Calculate the relative formula mass of ammonium chloride, NH4Cl.
(Relative atomic masses: H = 1, N = 14, Cl = 35.5)
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Relative formula mass = _________________________(2)
(Total 3 marks)
Q26.(a) Atoms are made of sub-atomic particles. Complete the six spaces in the table.
Name of sub-atomic particle
Relative mass Relative charge
_________________
___________
Neutron ___________ ____________
_________________ 1 ____________
(3)
(b) Complete the spaces in the sentences.
(i) The atomic number of an atom is the number of ___________________ in its
nucleus and is equal to the number of ___________________________ if the
atom is not charged.(1)
(ii) The mass number of an atom is the total number of _________________ and
___________________ in its nucleus.(1)
Page 25 of 33
(c) The table gives information about the atoms of three elements.
Name ofelement
Chemicalsymbol
Number of electrons in:
1st
shell2nd
shell3rd
shell
Fluorine F 2 7 0
Neon Ne 2 8 0
Sodium Na 2 8 1
Two of these elements can react together to form a chemical compound.
(i) What is the name and the formula of this compound?
Name __________________________ Formula _____________________(2)
(ii) What type of bonding holds this compound together?
______________________________________________________________(1)
(iii) Explain, in terms of electron transfer, how the bonding occurs in this compound.
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________(2)
(Total 10 marks)
Q27.The two carbon atoms represented below are isotopes.
ISOTOPE 1 ISOTOPE 2
14 mass number 12C C
6 proton number 6
(a) Describe two ways in which the isotopes are similar.
___________________________________________________________________
Page 26 of 33
___________________________________________________________________(2)
(b) Describe as fully as you can one way in which they are different.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(Total 4 marks)
Q28.You will find it helpful to use the information on the Data Sheet when answering this question.
In the nucleus of an aluminium atom are:
13 protonsand 14 neutrons.
(a) Complete these sentences.
(i) The mass number of the aluminium atom is ___________________ .
(ii) In an atom of aluminium there are ____________________ electrons.(2)
(b) Why is an aluminium atom electrically neutral?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(c) Complete the table for the element fluorine.
PARTICLE NUMBER OF PROTONS
NUMBER OF NEUTRONS
NUMBER OF ELECTRONS
Fluorine atom 9 9
Fluoride atom 10
(3)(Total 7 marks)
Q29.The formula for the compound hydrogen peroxide is H2O2.
Write down everything that the formula tells you about each molecule of
Page 27 of 33
hydrogen peroxide.
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________(Total 4 marks)
Q30.The information on the Data Sheet will be helpful in answering this question.
(a) Calculate the formula mass (Mr) of the compound iron (III) oxide, Fe2O3.
(Show your working.)
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(b) Calculate the mass of iron produced when 32g of iron (III) oxide is completely reduced by aluminium.
The reaction is shown in the symbol equation:
Fe2O3 + 2Al → 2Fe + Al2O3
(Show your working.)
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Answer = ___________________ grams(3)
(Total 6 marks)
Q31.The diagram shows one molecule of the compound ammonia.
Page 28 of 33
Write down everything that the diagram tells you about each molecule of ammonia.
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________
_______________________________________________________________________(Total 4 marks)
Q32.(a) Write down the symbols for
lithium ________________________________________
fluorine ________________________________________(2)
(b) The electronic structure of a lithium atom can be shown like this:
In a similar way, complete this diagram to show the electronic structure of a fluorine atom.
(1)
(c) A lithium atom can lose one electron to form a lithium ion which can be written (2)+
A fluorine atom can gain one electron to form a fluoride ion.
Choose from the list the correct way to write the fluoride ion.
Page 29 of 33
(2,6)+ (2,7)+ (2,7)- (2,8)+ (2,8)–
Answer _____________________(2)
(Total 5 marks)
Q33.This question is about lithium.
(a) A lithium atom has an atomic number of 3 and a mass number of 7.
Describe the atomic structure of lithium.
Include in your answer:• the number of each type of particle
• where in the atom each particle is found.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(4)
(b) (i) Name one other element with similar chemical properties to lithium.
Use the Chemistry Data Sheet to help you name the element.
______________________________________________________________(1)
(ii) Why are lithium and the element you named in part (i) classed as different elements?
______________________________________________________________
______________________________________________________________(1)
(Total 6 marks)
Q34.Lithium chloride can be used to colour flames dark red.
Page 30 of 33
By Alchimista (Own work) [CC-BY-SA-3.0] via Wikimedia Commons
(a) A chlorine atom has 17 electrons.
Complete the diagram to show the electronic structure of a chlorine atom.
(1)
(b) Lithium chloride (LiCl) can be made by reacting lithium with chlorine.
The electronic structure of a lithium atom is shown below.
Describe what happens to a lithium atom when the atom reacts with chlorine.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Page 31 of 33
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(3)
(Total 4 marks)
Q35.Scientists in the 16th century used the symbol shown in Figure 1 for gold.
Figure 1
Gold
The scientists thought platinum was made from gold and silver, so they used the symbol for gold in the symbol for platinum. The symbol for platinum is shown in Figure 2.
Figure 2
Platinum
(a) Gold and platinum are elements.
What is meant by the term element?
___________________________________________________________________
___________________________________________________________________(1)
(b) Why is it incorrect to represent platinum as shown in Figure 2?
___________________________________________________________________
___________________________________________________________________(1)
(c) Scientists now use a formula such as Ag2O to represent a substance.
What does the formula Ag2O tell you about this substance?
Page 32 of 33
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________(2)
(Total 4 marks)
Page 33 of 33
