Danyal Education
Group Properties Assignment 2 (Combined)
Unit 11
Group Properties in the
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Periodic Thble
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Multiple-Choice Qrestions
Which statement is likely to be correct about a new element (symbol Sa) with seven outer shell
electrons in its atoms?
A Its atoms form the ion Sa .
B It exists as a monatomic element.
C It conducts electricity.
D It forms covalent compounds with elements in Group I.
( )
2.
Fluorine is the element at the top of Group VII in the Periodic Table.
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Which statement is not true?
A Fluorine is less reactive than chlorine.
B Fluorine exists as diatomic molecules.
C Fluorine forms negative ions in its compounds.
D Fluorine displaces bromine from aqueous potassium bromide.
4.
Which electronic conflguration is that of a gaseous element that fills light bulbs?
A2
c 2.8.3
82.6
D 2.8.8
An atom of caesium, Cs, contains one electron in the outer shell. An atom of astatine, At,
contains seven electrons in the outer shell. Based on this information, it can be deduced that
caesium forms an acidic oxide
astatine forms a basic oxide
the two elements form the compound CsAt
the two elements are in the same period and same group
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A
B
C
D
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3.
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Sodium reacts with water to form an alkaline solution. What is the mass of sodium required to
produce 200 cm3 of an alkaline solution of concentration 1.50 mol dm-3?
A 3.30 g
B 6.90 g
C 10.29
D 13.89
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)
Structured Qrestions
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Xenon is an element in Group 0 of the Periodic Table.
(a)
What is the name given to this group of elements?
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(b) How many
(c)
Explain why the Group 0 elements exist as monatomic gases.
(d)
The Group 0 elements are unreactive. They do not combine with other elements.
However, chemists have successfully made certain Group 0 elements react to form
compounds. Tetrafluoroxenon, XeFo, is one such compound.
With the help of a 'dot-and-cross' diagram, explain the bonding in XeF..
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Chlorine, bromine and iodine are in Group VII of the Periodic Table. These three elements are
known collectively as halogens.
The halogens exist as diatomic molecules.
Use chlorine to explain the above statement.
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2.
electrons are found in the outer shell of a Group 0 element atom?
(b) (i)
Write down the formula of the halide ion that has the same electronic configuration
the argon
(ii)
atom.
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Write down the formula of the compound this ion forms with barium ion.
(iii) Write
the equation for the reaction to form the compound in
as
(b)(ii)
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(ii)
3.
What are the physical states of the three halogens?
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Explain the variation in the physical states of the three halogens.
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(c) (i)
Chlorine gas can be prepared by heating concentrated hydrochloric acid with solid potassium
manganate(VII).
KMnOo(s) + HC/(aq)
-
KC/(aq) + MnC/r(ag; + C/r(S) + HrO(/)
(a)
Balance the above equation.
(b)
Chlorine reacts with metals to form metal chlorides. In these reactions, chlorine acts as an
electron acceptor. Explain why chlorine atoms gain electrons in these reactions.
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(c)
Give the name and formula of the chloride formed when chlorine reacts with the following
metals.
potassium
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a
(i)
(ii) iron
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Chlorine reacts with non-metals to form non-metal chlorides.
Give the name and formula of the chloride formed when chlorine reacts with the following
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non-metals.
(i)
nitrogen
(ii) phosphorus
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The symbols and electronic conflgurations of Group I elements are shown in the following table.
Li
2.t
Sodium
Na
2.8.1
Potassium
K
2.8.8.1
Rubidium
Rb
2.8. 18.8. I
Caesium
Cs
2.8.18.18.8.
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Lithium
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Electronic configuration
Blement
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(b)
What is the position of caesium in the Periodic Table?
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(c)
Write the formula of the following compounds of rubidium.
(i)
rubidium nitrate
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Group I elements are powerful reducing agents
(i)
(ii)
Explain the term'reducing agents'
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(ii) rubidiumcarbonate
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(a) Why are these elements placed in Group I of the Periodic Table?
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How does the strength of the elements as reducing agents change down the group?
Explain your answer.
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The table below shows information about the elements in Group 0
Electronic
configuration
Relative
atomic mass
Boiling point
('c)
Dbnsity at r.t.p.
(g dm-')
He
2
4
-269
o.167
Ne
2.8
20
-246
0.833
40
-186
-152
Ar
Kr
2.8.18.8
84
Xe
2.8.18. 18.8
131
Rn
2.8.18.32.18.8
222
-107
1.61
5.46
9.25
(a)
Name the element with the symbol Xe.
(b)
Give the electronic configuration for argon.
(c)
Predict the boiling point of radon.
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(d)
Calculate the density of krypton at r.t.p.
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(e)
Explain the trend in the boiling points of the noble gases.
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Astatine is an element in Group VII of the Periodic Table. It has a proton number of 85 and
mass number of 210.
(a)
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Element
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5.
Use your knowledge of Group
VII elements to complete the table below.
Symbol
Number of valence electrons
Formula of hydrogen astatide
Formula of product of the reaction of astatine and iron
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(b)
The reaction between chlorine and iron is more vigorous than the reaction between astatine
and iron. Explain why this is
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Calculate the mass of product formed when 1 mole of astatine reacts with iron.
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Potassium superoxide, KO, can be used in spacecrafts to help astronauts breathe. It provides
oxygen by reaction with water according to the equation below.
4KO, + ZHrO--- 4KOH + 30,
The potassium hydroxide produced in the reaction is then used to absorb carbon dioxide breathed
out by the astronauts.
Calculate the mass of potassium superoxide required to produce 100 dm3 of oxygen,
measured at r.t.p.
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(a)
Potassium hydroxide, KOH, reacts with carbon dioxide to produce water and a potassium
compound.
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(c)
so.
(i)
Name the potassium compound.
(ii) Write the equation
for the reaction.
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(c)
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Elements in Group I of the Periodic Table are collectively known as alkali metals.
(a)
Using sodium as an example, explain why the Group I elements are known as alkali
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8.
Many spacecrafts carry lithium hydroxide, LiOH, to absorb carbon dioxide. Suggest one
advantage ofusing lithium hydroxide in place ofpotassium hydroxide for this purpose.
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metals.
(b)
Caesium is another alkali metal. It reacts explosively with water.
The reaction between caesium and water is more vigorous than the reaction between sodium
and water. Explain why this is so.
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(c)
13.3 g of caesium is added to water. What is the volume of 2.0 mol dm 3 hydrochloric acid
needed to neutralise the resulting alkaline
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solution?