A) Complete the statements given below-
By filling in the correct word in the blank from the word/s in the bracket.
1) The periodic table is based on the basic fundamental property___(atomic weight/ atomic number/electronic configuration).
2) Elements arranged in increasing order of atomic____.(numbers/weights)
3) ____horizontal rows called____ . (5/7/18/periods/groups)
4) ____ vertical columns called____ .(6/8/18/periods/groups)
5) Transition from _____to____character across a period. (metallic/non metallic)
6) Groups____& ____ subdivided into A and B.
7) Groups___ , _____ & ____ to ____ are called 'Normal -representative elements'.
8) Groups____ to____ are called 'transition elements'.
9) Group___ at extreme ____contains 'nobile gases'. (right /left)
10) ____elements are placed in group 1[IA] & 2[II A]. (reactive, metallic /reactive, non-metallic )
11) _____elements are placed in the upper right hand corner. (nonmetallic/metallic)
12) Periodicity in property i.e., recurrence in properties are seen with elements belonging to the same___(period/group/sub-group) in the periodic table after a difference of ___ , ___ , ____ , or (18/12/32/8) in atomic numbers due to recurrence of similar ______. (atomic weight/number of shells/valence electronic configuration)
13) Alkali metal Li, Na are present in group____ .
14) Alkaline earth metals Be, Mg are present in group____ .
15) Post-transition metal - Al is present in group____ .
16) Transition metal - Fe is present in group____ .
17) Transition metal -Zn is present in group _____ .
18) Lanthanide series are present in period____ .
19) Actinide series are present in period _____ .
20) The modern periodic law states that properties of elements are periodic functions of their ____(atomic mass/molecular mass/ atomic numbers)
21) The properties which reappear at regular intervals in the periodic table are called ____ . (atomic/ period/periodic properties)
22) ---- is one of the periodic properties, periodic in nature . (electronic configuration/ atomic radius/ electronic pull)
23) ____ is the energy required to remove an electron from the outer shell of a gaseous atom. (Ionization potential/electron affinity)
24) The unit of ionization potential is ____(mV/eV/iV)
25) _____ is the amount of energy released when an atom in the gaseous state accepts an electron to form an anion . (ionization potential/ electronegativity/ electron affinity)
26) Electronegativity is the tendency of an atom to attract____ to itself when combined in a compound. (protons/ electrons/ ions)
27) if the electronegativity difference between two combining atom is small the bond between them is _____. (electrovalent/ covalent/co-ordinate covalent)
28) An element is said to be____ if it loses one or more electrons when supplied with energy. (Non-metal/metal/metalloid)
29) The unit of atomic radius is _____ . (°C/A°/ eV)
30) A _____is formed from a metal by loss of elections. (Anion/cation/ proton)
31) Electron affinity of an atom is expressed in ____(A°/eV/mV)
32) An element 'X' gains an electron when supplied with energy. The electron configuration of X is_____. (2,8/2, 8, 1/2, 8,7)
33) Greater the tendency to lose electron/s the_____ the reactivity of the metal. (greater /lesser)
34) In the same period of sub group, increase or decrease in a particular (periodic) property is due to gradual charge in____. ( atomic weight/atomic size/ electronic configuration) in the arranged elements.
B) Name or State the following:
1) The number of electron shells in period- 1, 2 and 3 respectively.
2) The period number of the element 'X' having electronic configuration 2, 8, 8, 1.
3) The number of elements in the shortest period.
4) The number of short periods of the periodic table.
5) The metallic elements in the period-2 and period -3.
6) The non-metallic elements in period-2 and period-3.
7) The element in period-2 and period-3 having stable electronic configuration.
8) The element in period-3 having 5 valence electrons.
9) The element in period-2 having electronic configuration 2,4.
10) The period/s having 8 elements.
11) The element having one shell and one valence electron.
12) The period containing
a) rare earth elements
b) radioactive elements.
13) The bridge element in period-2 which has a diagonal relationship with aluminium in period-3.
14) A metalloid in period-3.
15) The valency of the elements in period-2
a) group 15[VA]
b) group 18[0].
16) The type of bonding of the chloride of the element in period-3, group-2[II A].
17) The type of bonding of the oxide of the element in period-3, group 13[III A] & 16[IVA].
18) The state of the chloride of the element in period-3 group 16 [VIA].
19) The character of the oxide of the element in Period-3 group 2[IIA] & 13[IIIA].
20) The character of the hydroxide of the element in period-3 group 2 [IIA].
21) The element in period-3 whose hydride is a strong acid.
22) Two properties trends of elements which increase from left to right in a period.
23) The number of valance electrons of the elements in group 1[IA] and in 2[IIA] .
24) The group number of the group having 3 columns of elements.
25) The group number to which lithium and sodium belong.
26) The group number to which magnesium and calcium belong.
27) The group containing highly reactive, non metals only.
28) The group number to which elements with 7 valence electrons belong.
29) The type of elements present in group 3 to 12 [II B to VIIB & VIII].
30) The group to which inert, unreactive elements belong.
31) The group to which the most reactive metals belong.
32) The two property trends which increase down a subgroup.
33) A non-metal in group 17 [VIIA] which is liquid at room temperature.
34) Two non-metals which react with group 17[VIIA] element forming liquid chlorides.
35) An element from group 1[IA] which reacts with an element of group 17[VIIA] forming a soluble electrovalent compound.
36) An element from group 1[1A] which dissolves in water to give caustic Potash.
37) A strong reducing agent from the elements - sodium of group 1[IA] and fluorine of group 17[VIIA] .
C) Select the correct elements in each case
1) Select the elements with the largest atomic radii u-
C, Be, N, F, Li
2) Select the element with the smallest atomic radii -
F, Ne, O
3) Select the element which has a higher electronegativity-
N, F, Cl
4) Select the element which has zero electron affinity-
C, Li, O, Ne
5) Select the element which show metallic character-
Na, Al, Si, P
6) Select the elements which show non-metallic character-
Be, C, Li, Cl
7) Select the elements which show metalloid character-
Be, B, C, N, F, Si
8) Select the elements which have three electron shells -
Li, B, Al, S
9) Select the elements which has the common valency 3-
Li, Be, B, C, Al
10) Select the element having the least electronegativity -
F, Cl, Br
11) Select the element having the smallest atomic size-
F, Cl, Br
12) Select the element having the largest atomic radii-
N, P, As(arsenic)
13) Select two elements whose electronegativity difference is large-
Na, C, Cl
14) Select two elements whose electronegativity is almost the same -
Li, F, Na, Ne
15) Select the element with the least electron affinity-
O, C, Ne, F
16) Select the element with the highest potential-
O, F, Ne
D) Arrange the following elements of the different periods-
as per the guidelines given below:
A ELEMENTS C O N Li F Ne B Be
B ELEMENTS Mg Si S Al Cl Na Ar P
1) According to their - decreasing atomic radii
2) According to their- decreasing ionization potential.
3) According to their- increasing electronegativity.
4) According to their- increasing electron affinity.
5) According to their- metallic, non metallic and noble gas character.
E) Arrange the following elements of different groups-
As per the guidelines given below:
A B
Na Br
K F
Li Cl
1) According to their - decreasing atomic radii .
2) According to their- increasing electronegativity.
3) According to their- decreasing ionization potential.
F) Match the Columns:
Column - A Column - Btomic
1) Atomic size-down a group a) No. of shekls, Nuclear charge
2) ionization potential-down a group b) nuclear charge, atomic radii
3) electron affinity- down a group c) No. of shells, nuclear charge
4) metallic character- down a group d) ionization potential, electron affinity
G) Select the current reason for each of the statement given below-
from the choice of reasons A and B.
1) Characteristic properties at definite intervals in the Modern Periodic Table
A: The Definite intervals are after difference of either 1 or 8 or 16 or 32 in atomic numbers.
B: The definite intervals are after differences of either 2 or 8 or 18 or 32 in atomic number.
2) Fluorine in group 17(VIIA) has a smaller atomic size than neon in group 18(0).
A: Outer shell in neon is completely filled, resulting in a form of repulsion.
B: Nuclear charge in fluorine atom is more than in the neon atom.
3) First ionization potential of an atom is less than the second ionization potential.
A: Energy required to remove 1st electron is more than required to remove 2nd electron.
B: Energy required to remove 1st electron is less than that required to remove 2nd electron.
4) Electron affinity of group 18(0) elements is zero.
A: Elements with stable electronic configuration find difficult to accept electrons .
B: Elements with stable electronic configuration find it difficult to lose electrons.
5) Elements with high gain electronegativity are usually non-metallic.
A: Non-metallic elements tend to gain electrons when supplied with energy.
B: Non-metallic elements tend to lose electrons when supplied energy.
6) Down a group, metallic characters increases since ionization potential decreases.
A: Nuclear attraction for valence electrons decreases & electrons are loosely held.
B: Nuclear attraction for valence electron increases and electron are strictly held.
7) Complete the table given by choosing the correct words-
from the list: decreases, increases, remains the same
A) Across- a period in a Periodic Table
a) Ionization potential
b) electron affinity.
c) electronegativity.
d) non-metallic character.
e) density and melting point
f) acidic nature of oxy-acids
B) Down- a group in a Periodic Table
a) ionization potential.
b) electron affinity.
c) electronegativity.
d) non-metallic character.
e) density and melting point.
f) acidic nature of hydrides.
Reason for increase or decrease in periodic properties :
C) Across - a period in a periodic table
a) Atomic size _____ because nuclear charge____., Number of shells _____.
b) ionization potential _____ because nuclear charge ____, atomic radii____.
c) non metallic character___ because ionization potential----, atomic radii___
d) electron affinity____ because, nuclear charge____, atomic radii_____
e) electronegativity____ because, atomic radii _____, nuclear charge ____
f) metallic character____ because, ionization potential ____, atomic radii____
D) Down - a group in a Periodic Table
a) Atomic size ____because number of shells___nuclear charge_____
b) ionization potential ____because atomic radii ___nuclear charge____
c) non metallic character____ because ionization potential_____ atomic radii____
d) electron affinity____ because, atomic radii____, nuclear charge _____
e) electronegativity ________because, nuclear charge____, atomic radii _____
f) metallic character____ because, atomic radii_____, ionization potential ____
8) State the salient features and the modern period table, with special reference to the arrangement of periods and groups in the periodic table. State how separation and periodicity of elements forms a special feature of the Modern Periodic Table.
9) State what are
a) periods
b) groups
c) Period number
d) group number in the Modern Periodic Table.
10) State the elements in correct order of increasing atomic numbers in periods 1, 2 and 3 of the Modern Periodic Table.
11) State the property trends of elements
a) from left to right in a period
b) on moving down a sub-group.
12) State the position of the following elements in the Modern Periodic Table
a) Normal or representative elements.
b) Bridge elements.
c) Transition and inner transition elements.
d) Alkali metals .
e) Halogen.
f) Noble or inert gases
13) Compare the 1(IA) group elements with 17(VIIA) group elements.
14) State what is mean by the terms
a) Periodicity in properties
b) Periodic properties.
15) Explain the terms :
a) atomic radii
b) Ionization potential.
c) electron affinity
d) electronegativity
e) metallic and nonmetallic characters of elements which suitable example.
16) With reference to the above periodic properties-
a) explain with reasons the trends in each of the periodic properties on moving
i) across a period
ii) down a sub-group.
Tabulate the same in the form of a chart.
17) Answer the following - using the correct symbols for the elements -
b) The element with the highest electronegativity from F, J, G, L.
c) The element from group-1 with the largest atomic size.
d) The electronic configuration of I.
e) The element with the least electron-affinity from C, D, G, L, K.
f) The element from J and K with a higher atomic size, giving a reason for the same.
g) The most reactive element from A, C, D and H.
h) The element with the highest nuclear charge from period -2.
i) The valency of element F.
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