Download Unit One Periodicity of Elements and their Properties

Unit One
Periodicity of Elements and their Properties
LESSONS(1-4)
Attempts of Elements Classification
Q1-Choose the correct answer:
1- Mendeleev arranged the elements of similar properties in
a- vertical periods . b. horizontal groups, c- vertical groups.
d. horizontal periods.
2. Moseley classified elements in his table in an ascending order according to their
a-. atomic Weights. b. atomic numbers. c-. chemical activity. d. valencies.
3. The number of elements in Mendeleev‟s periodic table is ……………… elements.
a. 67
b. 76
c. 92
d. 116
4. ………………….. l eft gaps in his table to be filled with suitable discovered elements in future
a- Moseley
b. Rutherford
c. Bohr
d. Mendeleev
5. The scientist who added zero group is
a- Mendeleev, b. Rutherford.
c. Moseley.
d. Bohr.
6. The scientist…………………..had discovered the main energy levels.
a. Moseley
b. Bohr
c. Hofmann
d. Mendeleev
7-.Elements of “p” block are arranged in ………………groups.
a-. two
b. five
c. six
d. eight
8. Which of the following elements locates in the third period 7
a-19K
b. I5P
c, 6C
d. 3Li
9. All of the following elements are located in group (2A) except
a-4Be
b, 20Ca
c. 11Na
d 12Mg
10. The element that its atomic number equals 17 is similar in its chemical structure to the element that its
atomic
number equals ………………,
a-.2
b.7
c.9
d.l9
11. The elements which have the same properties lie in the same………………… in the periodic table.
a-period
b. group
c. nucleus
d. energy level
12. The block that contains groups (lA) and (2A) in the periodic table is ………………….. b lock.
as
b. p
c. d
d. f
13. Which of the following elements lies in the same group in the periodic table?
a. Na,C
b. Na,Li
c. Na,Cu
d. Na.Ne
14. An element, its atomic number is (l8) , so it is considered ………………
a. a transition element.
b. an inert gas.
c. a metallic element.
d. a halogen.
B) Find the atomic number of each of the following:
l.An element exists in period 2 and group (6A).
2. An element exists in period 3 and group (lA).
3. An element exists in period 2 and group zero.
Q2) Write the scientific term:
1- Arrangement of the elements in an ascending order according to their atomic weights.
2. Arrangement of the elements in an ascending order according to their atomic numbers.
1. They are symbolized by K, L, M, N, O, P and Q letters.
2. . A block of elements which is located on the right side of the periodic table.
3. The block which contains the groups from (3A) to (7A).
4.
A kind of elements is symbolized by letter (B).
5.
They are symbolized by s, p, d and f.
6.
The block which contains the lanthanides and actinides.
7. The elements which occupy the middle block (d) in the periodic table.
…………………………………………………………………………………………………………………………
Q3 Complete the following statements : „
l. Mendeleev discovered that the properties of elements were repeated ………………….by the beginning of
each new ……………….
2-The atomic number of each element in Moseley‟s periodic table increases by .................. ….from the
preceding element in the same …………………………
3- ………………….., and …………………. scientists modified the Mendeleev‟s table.
4-In Mendeleev‟s table arranged the elements are arranged in …………………according to their atomic weight
5- Mendeleev arranged the elements ascendingly according to ……………………, while Moseley arranged
Them ascendingly according to ………………………..
6. Mendeleev explained his periodic table in his book ………………..
7.The number of elements which exist in nature is……………………..
8. Elements of “s” block are located on the ………………….. of the periodic table and they arranged in
………………….. groups.
9. The period number of the element equals the number of………………occupied by electrons in its atom.
10. The transition elements start from period ………………….. in the modern periodic table,
11. The modern periodic table consists of …………….. Horizontal periods and ………………. vertical groups
Q4) Answer the following:
1-What are the disadvantages of Mendeleev‟s table? (Mention two only).
2-What is the scientific principal upon which the elements are arranged in the modern periodic table
B) To who are these achievements attributed:
1-Corrected the atomic weights of some elements which were estimated wrongly
2-Added group zero to the periodic table
3- Discovered that the nucleus of the atom contains positively charged protons.
C) Locate the position of the following elements in the modern periodic table;
11Na - l8Ar` - 20Ca - 9F -
Q5-Put ( ) or (X),then correct what is wrong :
1-The elements which have similar chemical and physical properties are put in horizontal periods.
2- Scientists classified the elements in order to facilitate their study.
3- Mendeleev had to put more than one element in one place.
4-Rutherford had discovered the main energy levels of the atom.
5-the elements are arranged in Mendeleev‟s table in an ascending order according to the increase in the
atomic number.
6-Moseley puts lanthanides and actinides on the left side of the periodic table.
7. The modem periodic table consists of three blocks of elements,
8. The period number of the element equals e number of electrons in the outermost energy level in its atom.
9 .The atomic number of an element increases from an element to the next element in the period by one.
Q6) A- Give a reason for:
1- Scientists thought to classify elements according to their properties.
2-Elements of the same group have similar properties.
3-Mendeleev left gaps (spaces) in his periodic table.
4-Moseley arranged elements in an ascending order according to their atomic numbers
5-Elements of the same group have similar properties.
6-Scientists cannot discover a new element between sulphur (16S) and chlorine (17CI).
7- In periods, by increasing the atomic number, the atomic size decreases.
8 .By increasing the atomic number within groups, the atomic size increases.
LESSON 2
Q1-Complete the following:
1- ln periods, by increasing the atomic number, the atomic size ……………………. While the
electronegativity ……………………………
2-…………………….It is the ability of the atom in covalent molecule to attract the electron of chemical bond
towards itself.
3-…………………….has the highest electronegativity which equals ………………………..
4- ………………………is a polar compound because the difference in ……………………..between its
elements is relatively …………………………..
5-In the same period, the element which has the highest electronegativity lies in the group………………..
6-In anmonia molecule. …………………………atom
than………………
atom as it has higher …………………….
attracts
the
electrons
of
the
bond
more
. 7- From examples of polar compounds are ……………….. ; and…………………, while from non-polar
Compounds are …………………………..and …………………………….
8-During chemical reactions, atoms of metals tend to ………………………..electron(s) and change into
...............
which carry a number of positive charges equal to the number of lost ……………………
9- Silicon (14Si) is a ............... element which has the properties of .................... and ……………………..
10- By increasing the atomic number within a period, the metallic property ………………….while the
nonmetallic
property .............................
11- The most metallic element in group (lA) lies at the ………………………… , while the least metallic
element lies at the ………………………of the group.
12- There is ............................. relationship between the …………………of an element and its nonmetallic
property'
13-Each period in the modern periodic table starts with …………………. elements.
14 Some metal oxides dissolve in water giving …………………….which turns litmus solution into
……………..
15. Sodium reacts with water and ……………….. gas evolves which ………………... with a ............... sound.
16……………………. and …………………… are metals which don‟t react with water.
17. When magnesium oxide dissolves in water, it gives,…………. , while carbon dioxide dissolves in water
giving
………………………...
18. Basic oxides are formed by the reaction of …………………..with oxygen, while acidic oxides are formed by
the
reaction of …………………… with oxygen.
19. CO2 + H2O
20. Mg + 2HCl
Q2) G.R:
1- The atomic size of sodium (11Na) is greater than that of magnesium (12,Mg),
2-In groups, by increasing the atomic number, the atomic size increases.
3-Ammonia is considered a polar covalent compound.
4-Methane and hydrogen sulphide are not considered from polar molecules.
5-Water is more polar than ammonia.
6. Cesium is considered one of the strongest metallic elements.
7. Fluorine is considered one of the strongest nonmetallic elements.
Q3) The opposite figure represents part of the periodic
1. Which element has the highest electronegativity?
2. Which element has the greatest atomic size?
3. If the electronegativity of (H) equals 2.1 and that of (N) equals 3,
calculate
the polarity (the difference in electronegativity) in ammonia.
Q5) Write the scientific term:
1. The measuring unit of atomic radius.
2. They are covalent compounds in which the difference in electronegativity between elements forming
their
molecules is relatively high
3. There is a direct relationship between the atomic size of the atom of an element and its
electronegativity.
4. Fluorine has the least electronegativity which equals 4.
5. Methane and hydrogen sulphide are from polar compounds.
6. Elements which have less than 4 electrons in their outermost energy level.
7. An atom of nonmetallic element that gains one electron or more during the chemical reactions.
8. The strongest nonmetal in group (7A)
Q6) Put (\/) or (X), then correct what is wrong:
l. In periods, by increasing the atomic number, the atomic size decreases.
2.There is a direct relationship between the atomic size of the atom of an element and its electronegativity.
3. Fluorine has the least electronegativity which equals 4.
4. Methane and hydrogen sulphide are from polar compounds
5-The number of electrons in positive ion is greater than that of its atom.
6-Each period ends by a nonmetal element.
7, The metallic property decreases in group (IA) as we go from the top to the bottom.
8-The electronegativity increases in groups by increasing the atomic number.
9-Non-metal oxides are considered basic oxides
Q7) Choose the correct answer:
l. All of the following ions have the same electronic configuration of neon (10Ne) except
+3
+
+
+2
a.Al
b. Na
c. Li
d. Mg
2. An element (X), its atomic number is I5 so, the number of electrons in its ion equals
a.10
b.l5
c.l7
d.l8
3. By increasing the atomic number within a period, the
a. metallic property increases.
b. metallic property decreases.
c. nonmetallic property decreases. d. atomic size increases.
4. An element (Y), its atomic number is 13 so, the electronic configuration of its ion is
a.2,8
b.2,8,3
c.2,8,8
d.2,8,8,3
5. All of the following elements are from semi-metals except
a. tellurium.
b. silicon. c. boron. d. bromine.
6-All of the following elements don‟t react with dilute HCl except
a.Cu
b. Zn
c. S
d. C
7 - ,Atl of the following are related to CO2 except
a-it is acidic oxide.
b. it is nonmetal oxide.
c-its solution turns litmus to red
. d. its solution turns litmus to blue.
8- Metal oxides are …………………….. oxides.
a- acidic
b. basic
C, neutral
9- Sodium oxide is from ,………………. oxides,
d. amphoteric
a-amphoteric
b. acidic
c. nonmetallic
d. basic
Q8) What is meant by
1-Non-metals: 2. Metalloids:
3-Chemical activity series
5-Acidic oxides
. Q9) Look at the following figures, then answer the following questions :
Fig. (A)
Fig. (B)
l . Which of the previous figures represents.
1- A positive ion
2. A neutral atom
.
2-Determine the position of the atom in the periodic table (period - group) :
.
Q10) Choose the odd word out, then write the scientific term of others
1-. Boron / Silicon /Arsenic / Bromine / Tellurium.
+3
+
+2
2- AL /Na / Mg / CL / O-2r
3. Silver/ Sodium / Iron / Calcium.
4. SO2 /MgO/Na2O/CaO
LESSON 3
Q1) Write the scientific term :
1-Elemtents which are located at the left side of the periodic table
2-Themost active element
3 - The halogen which exists in a liquid state.
4. Rays which are emitted from cobalt (60).
Q2) Choose the correct answer
1-Elements which have atomic numbers……………………… are called alkali metals
a- 2,8,16
b.2,l0,l8
c.3,11,l9
d.4,l2,20
2-metals have the following properties except …………………….
a-They have low density.
b- they conduct electricity,
c-They conduct heat.
d. they don‟t react with water.
3-……………..form positively charged ions when they enter the chemical reaction.
a-Inert gases
b. Nonmetals c. alkaline earth metals
d. Halogens
4- Sodium reacts with water……………….. gas evolves.
a- O2
b.CO2
c.H2
d.NO2
5- ………………..are kept under the surface of kerosene in the lab.
a- Alkaline metals
b. Halogens
c. lnert gases
d. Alkaline earth metals
6-The most fist active element in group (lA) is ...............
a- Na
b. Cs
c. K
d. Li
7. All of the following elements are alkaline earth metals except …………………
a- 4Be
b. 12Mg
c. 19K
d. 20Ca
8. The chemical activity of ……………….... element is more than that of 38Sr_
a-.4Be
b. I2Mg
c. 20Ca
d.56Ba
9. Alkaline earth metals react with water and …………………….. gas evolves.
a-.H2
b.O2
c.N2
d-.He
10. The element that forms a positive ion which carries two positive charges during chemical reactions is
.
a- .Na
b- Mg
c- K
d- Li
11. The strongest element of alkaline earth metals in the reaction with water is ...___
a- magnesium. b. calcium.
c. barium.
d. sodium.
Q3) G.R
1-Elements of group (1 A) are known as alkali metals.
2-Sodium and potassium are kept under surface of kerosene
3-Rubidium and cesium elements sink in water
4-The reaction of potassium with water is stronger than that of sodium.
.5- The chemical activity of alkaline earth metals increases by increasing their atomic size.
6-. Sodium (11Na) is more active than magnesium (l2Mg).
Q4)Complete the following statements :
l. Lithium element ……………………water surface as its density is ……………………..than that of water.
2. During the chemical reactions , sodium tends to ……………….. an electron and changes
into…………………..
ion which carries positive charge.
3. Potassium reacts with water giving ………………….. and ………………… gas evolves.
4. The chemical activity of alkali metals _,,.,,,..,,,,.. as the …………….. increases.
5. When sodium reacts with water………………………… gas evolves.
6. ……………….._ metals are elements of group (QA) which are located on the ……………………….
of the periodic table
7. During chemical reaction, alkaline earth metals tend to ……………………… their valency electrons
and change into ……………………. ions which carry……………………….
8, The valency of magnesium (l2Mg) is …………………… because it has …………………….electron(s)
in the outermost energy level,
9-Halogens lie in group …………………..
10-……………….and……….. are halogens which exist in gaseous state.
11-……………………….,.is used in food preservation.
12- Silicon is used in manufacture of …………….. , while liquefied nitrogen is used in ……………………..
Q2) Compare between alkali metals and alkaline earth metals 2
Alkali metals
Alkaline earth metals
Q5) Put (
) or (X) . then correct what wrong : `
l . Alkaline earth metals are less active than alkali metals.
2. Alkaline earth metals are located in the second group of “p” block elements. 1
3. Magnesium is less active than calcium , while it is more active than barium.
4. Alkali metals are bad conductors of heat.
5. Magnesium sinks in water. „
6.l Halogens are univalent elements.
7. Boiling point of liquefied nitrogen is (-l96°C).
8. Bromine is a halogen which exists in a solid state.
Q6)
The opposite figure represents group (IA) oi' the periodic table. Answer the following questions
l . The element which has the electronic configuration (2, 8. 8. l) is ……………………..
2, The most metallic element is ………………………
3. Elements which float on the water surface are ……………………, `
4 The least metallic element is ………………………………
Q7) „Which of the following elements 11X, 17Y, 14Z
l. Can replace iodine in potassium iodide solution :
2. Used in the manufacture of electronic slides
3. Can react together and form salt
Q8) Mention one use for each of the following:
l. Silicon slides
2. Liquid sodium
3. Cobalt 60
Q7)Complete the following equations.
l . Br2 + NaCl
2. CL2 + 2KI
3. 2K + Br2
Q8) Choose the odd word out, then mention the scientific term for the rest
l, Potassium/ Iodine / Fluorine / Astatine / Bromine.
2. Fluorine / Chlorine/ Oxygen/ Hydrogen / Sodium.
„
(5) Some elements in the periodic table are
represented by the letters from A to E
and are included in the simplified table
asshown below :
1. Choose the letter(s) which indicates :
(a) A halogen,
(b) The most active metal.
(c) An alkaline earth metal.
2. Write the chemical equation which represents the reaction of Water with element “A”
3. Complete:
A
B
C
D
E
(a) The molecule of element D consists of ………………
(b) The valency of element F is ………………. and that of element D is ……………………
(C) The density of element B is ……………………. than that of element A.
Lesson 4 –Questions
Q1)Choose the correct answer :
1 - The largest percentage of consuming water internationally is used in
a- industrial fields.
b. personal fields c-_ agricultural fields .
d (a) and (b).
2. All of the following are from water properties except
a- it exists in 3 states.
b. it has high latent heat.
c- it is used in generating electricity,
d. it is a non-polar compound.
3, Water molecule consists of
a- two atoms of three different elements.
c- three atoms of three different elements.
b. three atoms of two different elements
d. four atoms of two different elements.
Q2) Mention the importance of water (two only).
Q3) complete the following statements ;
1- South America is the largest continent in consuming water in ………… while ......,,....... is the largest
continent
in consuming water in agricultural fields,
2- Water is considered as a good ………………………… solvent , as it dissolves most
……………compounds.
3-Tie density of water in ………………….. state is lower than its density in …………………….. state.
4-Wlater molecule consists of ………………………… atoms and …………………….. atom.
5-The bond between water molecules is called ……………………….. bond.
6-teasing the boiling point of water is due to………………….. ...,..
7-Mixing of animals and human Wastes with water leading to the infection by many diseases such as
…………………………….. , …………………………
and …………………………..
8. Increasing the mercury concentration in drinking Water causes ………………………… while arsenic
increases the infection rate by ………………………………….
9. We must ………..... the drinking water tanks and don‟t store the tap water in ………………. bottles.
10. Eating fishes contain high concentration of lead cause the ………………… of brain cells. .
11. The nuclear reactors cause both ………………..and ………………… pollution for Water.
„
Q4) Mention what is happened in these cases?
1-The temperature of water decreases than 4°C.
2- Decreasing the value of latent heat for water.
3-Decomposing water into its elements by heating
.
Q6) Put ( \/) or (X) ,then correct what is wrong :
l, Table salt and sugar are from covalent compounds.
2.The angle between the two covalent bonds in water molecule is l04.5°
Q7) Write the scientific term :
1-The bond between hydrogen atom and oxygen atom in water molecule.
2-The bond which links the molecules of water
;
3-A kind of Water pollution which results from mixing of humans and animals wastes with Water.
4-, A kind of Water pollution which results from discharging of factories residues and sewage in rivers and
seas
5-A Water pollutant which causes the death of brain cells. Q What is meant by water pollution?
6-The positive pole of Hofmann‟s voltameter.
7-. Ions responsible for the basic property in water molecule
Q8) Give reasons for :
l. Ice floats on water surface.
.
2.The high boiling point of water.
.
3. The closed glass bottle filled with water is broken when it is put in freezer.
4. Water is important liquid in extinguishing fires.
5. Sugar dissolves in water although it is a non-polar compound.
6.Water has neutral effect on both litmus papers.
7.Adding g drops of dilute acid to water during its electrolysis,
8 during water electrolysis. oxygen gas evolves above the anode.
9.During water electrolysis. the volume of the gas evolved at the cathode doubled the volume of the gas
evolved at the anode
.
Q10) Explain what happens when.
l. Adding a detergent to a pool containing green water and fish. Why?
2.Increasing the temperature of some water areas which are used in cooling the nuclear reactors. Why?
3, Storing the tap water in empty plastic bottles.
4. Water is polluted by the Wastes of man and animal.
Q12) Put. (v) or ( X) , then correct the wrong :
1. Eating food containing high percentage of lead causes hepatitis.
2. Adding of agricultural fertilizers to water causes water pollution.
3, Storing the tap water in plastic bottles causes the increase of infection with hepatitis