A) FILL IN THE BLANKS :
1) The serial number of an element in the periodic Table is also its.....
2) The metallic character.... in a Group as one moves from top to bottom.
3) The metallic character... in a Period as one moves from left to right.
4) ....is the most active nonmetal.
5) ....is the most active metal.
6) An increase in nuclear charge... the tendency of an atom to accept electrons.
7) The atomic size....as one moves from left to right across a Period.
8) The element in Group VIIA which is a liquid at room temperature is....
9) Nuclear charge of an atom is the... charge on the nucleus of an atom, equivalent to the atomic...of an atom.
10) Atomic size of neon is...than the atomic size of fluorine.
11) With increase in nuclear charge the nuclear attraction for outer electron..... . Hence ionisation potential......
12) If an element has one electron in its outermost shell. Then it is likely to be.....
13) The Properties of elements are periodic function of their....
14) The element below sodium in the same Group would be expected to have a..... . electronegativity than sodium and the element above chlorine would be expected to have a..... . ionisation potential than chlorine.
15) On moving from left to right in a given Period, the number of shells..
16) On moving down a Group, the number of valence electrons.......
B) Choose Correct Option:
1) The chemical properties of an element depends on its:
a) atomic mass
b) atomic number
c) atomic energy
d) atomic volume
2) Total number of vertical columns (Groups) in the Long Form of the Periodic Table is :
a) 8 b) 18 c) 17 d) 16
3) The element having the lowest ionisation potential in period 3 is:
a) Na b) K c) Mg d) Al
4) The number of elements present in Period 3 is :
a) 6 b) 32 c) 18 d) 8
5) On going down a Group, the number of valence electrons.
a) increases b) decreases
c) remains the same
d) varies irregularly
6) The number of Periods in the Long Form of Periodic Table is:
a) 6 b) 7 c) 8 d) 10
7) On moving down a Group, the size of atoms :
a) increases b) decreases
c) remains the same
d) varies irregularly
8) Which one of the following ions has the smallest radius ?
a) Cl⁻ b) K⁺ c) S²⁻ d) Ca²⁺
9) On moving from left to right in a Period the metallic character of elements:
a) increases
b) decreases
c) remains the same
d) varies irregularly
10) The correct order of decreasing first ionisation potential is :
a) C > B > Be > Li
b) C > Be > B > Ki
c) B > C > Be > Li
d) Be > Li > B > C
11) Which halogen has the highest electron affinity ?
a) F b) Cl c) Be d) I
12) The most electronegative element in the Period Table is:
a) N b) O c) Cl d) F
13) Which has the smallest size?
a) Na⁺ b) Al³⁺ c) Mg²⁺ d) P⁵⁺
14) Which of the following is the correct order of ionisation potential in the Periodic Table?
a) F > O > N > C
b) O > F > N > C
c) O > N > F > C
d) C > N > O > F
15) The electron affinity for noble gases is likely to be:
a) high b) small c) zero d) Positive
16) Which of the following has the highest electron affinity?
a) F b) O c) O⁻ d) Na⁺
17) The size of a positive ion is:
a) more than its atom.
b) less than its atom
c) equal to its atom
d) none of the above
18) Which one of the following is correct order of the size ?
a) I > I⁻> I⁺
b) I > I⁺> I⁻
c) I⁺ > I⁻> I
d) I⁻ > I > I⁺
19)The size of chloride ion (Cl⁻) is
a) smaller than chlorine atom
b) bigger than chlorine atom
c) equal to that of chlorine atom
d) none of the above
20) The ionic radii of N³⁻ , O²⁻ , F⁻ and Na⁺ follow the order
a) N³⁻ > O²⁻ > F⁻ > Na⁺
b) N³⁻ > Na⁺ > O²⁻ > F⁻
c) Na⁺> O²⁻ > N³⁻ > F⁻
d) O²⁻ > F⁻ > Na⁺ > N³⁻
B) NAME THE FOLLOWING:
1) The element present in the first Period.
2) The biggest atom in the third Period.
3) The smallest element of third Period
4) The family of elements to which chlorine belongs.
5) The family of elements to which sodium belongs.
6) The family of elements to which argon and neon belongs
8) Least electronegative element of halogen family.
9) A non metal which has three electrons in its outermost shell
10) The smallest atom in the third Period
11) The least reactive elements in Group IA.
12) The most metallic element in the third Period.
13) The most nonmetallic element in the third Period
14) The element which is most electronegative in the third Period
15) A greenish yellow gas other than chlorine..
16) The most abundant halide salt.
17) The element which has the highest ionisation potential.
18) The element of third Period which has least ionisation potential
19) The most electronegative element of second period
20) An element in period 3 with electronegativity 3.0
21) The element with the least ionisation potential in the 2nd period.
22) The element which has the highest electron affinity in the third Period
23) The noble gas having an electronic configuration 2,8,8.
24) The valency of elements in Group I.
25) An element of group VIIA, solid at room temperature.
C) TRUE/FALSE
1) The electron present in the outermost shell are called valence electrons.
2) In a group, atomic and ionic radii decrease from top to bottom due to increase in the number of shells.
3) The electron affinity of elements increases in a group from top to bottom and decreases along a period from left to right.
4) The amount of energy required to remove a loosely bound electron from the outermost shell of an isolated atom is called ionisation potential.
5) Electron affinity is the property of an atom to attract electrons towards itself, when combined to form a compound.
6) Lithium resembles radium and potassium in electropositive character and univalency.
7) The element in a Group have consecutive atomic Numbers.
8) On going down in a group of the Modern Periodic table, the metallic character of elements increases.
9) The tendency of an atom of an element to donate or lose electrons is called electropositivity.
10) Iron is a non-metal.
D) DEFINE:
1) Periods in Periodic table
2) Group in Periodic table
3) Periodicity
E) ANSWER THE FOLLOWING:
1) How many electrones are present in the valency shell of the element with the atomic number 18
2) From amongst Be, B, and C, choose the element with the highest ionisation potential
3) What is similar in the electronic structure of Li, Na, and K
4) Which of the following elements are in the same Group of the Periodic table. Magnesium, nitrogen, beryllium, sulphur
5) Which group of elements was missing from Mendeleev's original Periodic table
6) State the Periodic law on which Mendeleev's Periodic table was based
7) What similarity do halogen show in their molecular state
8) If an element is in Group 7(or group 7A) is likely to be metallic or nonmetallic in character
9) Predict the group of an element X if it's atomic number is 16.
10) Select the correct order f radii of three species Ca, Ca⁺ and Ca²⁺
11) The elements lithium, sodium and potassium were put in one group on the basis of their similar properties.
a) What are those similar properties
b) What is the usual name of this Group or family.
13) What is the cause of periodicity of elements in the Periodic table.
14) In which part of a Group would you separately expect the elements to have:
a) the greatest metallic character
b) the largest atomic size
14) a) What are alkali metals?
b) In which Group and subgroup are they placed ?
c) What is their valency
d) Why do they not occur free in nature?
15) a) What are noble gases?
b) what is the speciality of their outermost shells
c) Why is that group referred to as Zero Group
d) Why are they referred to as inert gases ?
F) REASON BEHIND:
1) Why electron affinity of atoms increases from left to right along a period in the Modern Periodic table
2) Why the elements with low ionisation potential exhibit metallic character.
3) Sodium is referred to as a normal element.
4) Sodium and potassium are placed in group I
5) Electron affinities of two elements A and B are as follows
A=3.79 eV and B= 3.56 eV which of them will ionise more easily and why ?
6) Which is larger, Na⁺ or K⁺ ? Why?
7) Why is the electron affinity for F Less than that of Cl?
8) Why electron affinity of halogen is comparatively high
9) Ionisation potential of alkali metals is comparatively low.
10) Why is chlorine more reactive than bromin ?
11) Why Potassium is more reactive than sodium.
12) Why is ionisation potential of O is less than that of N
No comments:
Post a Comment