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WorksheetsPeriodicity II
Total questions: 40
Worksheet time: 30mins
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
decreases, increases
increases, increases
increases, decreases
stays the same, increases
P, Cs, Co, Sr
Which of the following will have a higher electronegativity than arsenic (As)?
Carbon (C)
Neon (Ne)
Antimony (Sb)
Germanium (Ge)
The element with the lowest electronegativity in Period 3 is -
Na
Cl
Ar
Mg
The electronegativity of Cl is the highest in Period 3. Why?
Cl is the largest and has the greatest effective nuclear charge
Cl is the smallest and has the lowest effective nuclear charge
Cl is the largest and has the lowest effective nuclear charge
Cl is the smallest and has the greatest effective nuclear charge
Which of the following is true for the elements in the Periodic Table?
There are fewer metals compared to non-metals.
The size of the atoms increases with increasing nucleon number.
The metallic property increases on going down a group.
The reactivity increases on going down a group.
The first ionisation energy generally increases across a period in the Periodic Table. Which statement explains why the first ionisation energy of sulphur is lower than that of phosphorus?
The electrons in the p orbitals of sulphur experience greater electrostatic repulsion than that of phosphorus
The sulphur atom has more electrons than phosphorus atom.
The S-S bond is weaker than the P-P bond.
The size of S8 molecule is bigger than P4 molecule.
The acid-base properties of oxides are related to their structure and chemical bonding. Which oxide dissolved in water to form an acidic solution?
MgO
Al2O3
. SiO2
SO3
Which statement explains the difference in the first ionisation energies between beryllium and boron?
Boron atom has more valence electrons.
Boron atom has a greater shielding effect.
Beryllium atom has a more stable electronic
configuration.
The 2p electron in boron atom is at a higher
energy level than the 2s electron in beryllium atom
The compounds Na2O, Al2O3 and SO2 respectively are
acidic, amphoteric and basic.
amphoteric, basic and acidic
basic, acidic and amphoteric
basic, amphoteric and acidic
Which properties are typical of most non-metals in period 3?
I. They form ions by gaining one or more electrons.
II. They are poor conductors of heat and electricity.
III. They have high melting points.
I and II only
I and III only
II and III only
I, II and III
Which factors lead to an element having a low value of first ionization energy?
I. large atomic radius
II. high number of occupied energy levels
III. high nuclear charge
I and II only
I and III only
II and III only
I, II and III
Which statement about electronegativity is correct?
Electronegativity decreases across a period.
Electronegativity increases down a group.
Metals generally have lower electronegativity values than non-metals.
Noble gases have the highest electronegativity values.
Which compound of an element in period 3 reacts with water to form a solution with a pH greater than 7?
SiO2
SiCl4
NaCl
Na2O
Which equation represents the first ionization energy of fluorine?
F(g) + e– --> F–(g)
F–(g) --> F(g) + e–
F+(g) --> F(g) + e–
F(g) --> F+(g) + e–
Which of the following causes ionisation energy to increase when going across period 3 from left to right?
I. Increase in shielding effect
II . Decrease in atomic radius
III. Increase in nuclear charge
II and III only
I only
I and II only
I,II and III
How many valence electrons does the element have?
E1 = 943
E2 = 1,950
E3 = 3,852
E4 = 5,492
E5 = 23,085
E6 = 26,791
E7 = 30,024
1
2
3
4
5
What makes the d block wider than either the s block or the p block?
The d sub-orbital can hold ten electrons, making the d block ten elements wide.
The d block is the most researched area of the periodic table.
The elements in the d block are more important than the elements in the rest of the table.
The elements in the d block are all metals.
Element X is in Period 2 of the Periodic Table. The first seven successive ionization energies of element X is given below
1400, 2860, 4580, 7480, 9440, 53 270, 64 360
Choose the statement that is not true about X.
Element X exist as a liquid at room temperature and pressure at 1 atm.
Atom X has three unpaired electron in its valence configuration.
The electron affinity of atom X is endothermic.
Element X is a nonmetal.
The reduction of force of attraction between nucleus and valence electrons by the electrons present in the inner sub-shell is called ____________.
Electron affinity
Electronegativity
Shielding Effect
Periodicity
Which of the following elements you expect to have greater shielding effect?
Li
Na
K
Rb
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
decreases, increases
increases, increases
increases, decreases
stays the same, increases
Based on the successive ionisation energies below,how many valence electrons does the element M have?
IE1 = 943
IE2 = 1,950
IE3 = 3,852
IE4 = 5,492
IE5 = 23,085
IE6 = 26,791
IE7 = 30,024
2
3
4
5
Why does ionization energy decrease going down a group?
Adding more energy levels makes the valence electron further from the nucleus
There are more valence electrons in the outer shell
There are more protons in the nucleus
There are less protons in the nucleus
Elements P, Q and R have 18, 19 and 20 protons respectively.
It is found that the atomic size of P is the smallest. What is the factor that influences its size?
Least number of shells.
Smallest number of protons.
Smallest relative atomic mass.
Largest effective nuclear charge.
Element with the greatest second ionisation energy is
argon
calcium
chlorine
potassium
The first seven ionisation energies of element M are 786, 1577, 3229, 4356, 16080, 19790 and 23780 kJ mol-1. In the Periodic Table, element M is in group
3
4
12
14
The data below shows the values of the first to the fifth ionisation energy of element X.
Ionisation energy kJ mol-1
First 577
Second 1820
Third 2740
Fourth 11600
Fifth 14800
The configuration of valence electrons of element X is:
s2
s2 p1
s2 p3
s2 p4
An element Z has the electronic configuration as follows:
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p5
Which of the following statements is (are) TRUE?
I Element Z is a metal in d-block.
II. Element Z is in period 4 in the Periodic Table.
III. Element Z tends to form ion with a charge of -1.
I and II
II and III
I and III
All
Across period 3 from Na to Cl, the first ionisation energy increases because
I. the number of protons increases
II the electronegativity of the elements becomes smaller
III the number of shells occupied by electrons increases
I
I and II
II and III
All
Arrange these in increasing order of electronegativity:
F, N, B
B < N < F
B < F < N
N < F < B
F < N < B
