perodic classification

Question 1

s block electronic config

Answer 1

ns^1-2

Question 2

group 1 elements are known as

Answer 2

alkali elements

Question 3

group 2 are knows as

Answer 3

alkaline earth elements

Question 4

p-block config

Answer 4

ns^2np^1-6

Question 5

elements who show diagonal relationship

Answer 5

li with mg , be with al, b with si

Question 6

d-block config

Answer 6

(n-1)d^1-10ns^0-2

Question 7

IONIC radius

Answer 7

ionic radii>neutral atom , radii directly propotional negative charge,

Question 8

what is ionization enthalpy

Answer 8

enegry required to remove an outermost electron from an ground atom to form cation

Question 9

trend in ionization enthalpy

Answer 9

IE increases left to right and decreases down the group,but half & fully filled orbitals are more stable ho high IE, IE inversly to atomic size ,charge directly to IE,
IE1 of group 2 element > of grp 13

Question 10

what is electron enthalpy

Answer 10

energy released when an electron is added to an atom

Question 11

trend in electron gain enthalpy

Answer 11

EGE increses left to right, and decreases down the group, it is inversly to atomic size , directly to nuclear charge , half and fully filled EGE will be less

Question 12

what is electronegativity

Answer 12

tendecy of an atom to attaract shared pair of electron towards itself, only depend upon nuclear charge or size

Question 13

trend in electonegativity

Answer 13

left to right increases, down the group decreases

flourine is the most electronegative element

Question 14

metallic character

Answer 14

will decrease from left to right

increases down the group

Question 15

chemical reactivity for metals

Answer 15

invesely to IE,EN directly to atomic radii

Question 16

reactivity for non-metals

Answer 16

directly to EN,ege and inversely to atomic radii

Question 17

trend of chemical reactivity

Answer 17

down the group ,metals reactivity increases and non metal decreases , across the group metals reactivity decreases, non metal increases

Question 18

reducing character

Answer 18

increase down the group,decrease across period

Question 19

oxidizing character

Answer 19

decrease down the group, increases across the priod

Question 20

oxides

Answer 20

M+02—->MxOy

Question 21

non-metals

Answer 21

Hydrogen (sometimes)
Carbon.
Nitrogen.
Oxygen.
Phosphorus.
Sulfur.
Selenium.
Fluorine
bromine 
iodine

Question 22

acidic

Answer 22

the oxide which form acid on hydrolysis

usually non-metals oxides are acidic in nature

Question 23

basic

Answer 23

the oxide which form base on hydrolysis

usually metal oxides form base

Question 24

amphoteric

Answer 24

the oxide which doesn’t react with H2O but can react with both acid and base
eg:Al203

Question 25

neutral

Answer 25

this oxide doesn’t react with anything
C0(carbon monooxide)
NO(nitric acid)

Question 26

ionization potential

Answer 26

it is the minimum amount of energy required to remove an outermost loosely held electron from isolated gaseous atom

Question 27

successive IP

Answer 27

when any element remove more than 1 electron , nucleus increases charge to hold remaining electron
so the successive IP gets exceptionally high

successive IP∝ energy required
no of electron ∝ 1/z-eff

Question 28

most stable electron configuration

Answer 28

ns^2np^6–> noble gas config.

Question 29

factors affecting IP

1. atomic size or atomic radii

Answer 29

down the group ∝ no of shell increases 
IP∝1/no. of shell 
IP DECREASES DOWN THE GROUP
across the period ∝no of electron 
electron increases ∝1/size 
IP INCREASES ACROSS THE PERIOD

Question 30

factors affecting IP

nuclear charge

Answer 30

down the group ∝ 1/nuclear charge

across the period ∝ nuclear charge

Question 31

factors affecting IP

penetration power

Answer 31

highest penetration power or IP required to remove electron is s>p>d>f

Question 32

factors affecting IP

electronic configuration

Answer 32

half-filled and fully filled orbital are exceptionally stable. Due to symmetric distribution

Question 33

exception of IP

Answer 33

shielding and screening effect

IP of 4th period > IP of 3rd period

Question 34

electron gain enthalpy

Answer 34

it is the minimum amount of energy required or released when an electron is added
negative means energy is released
positive means energy is absorbed
this concept of electron gain is mostly applicable for non metals bcoz they have a tendency to accept electrons

Question 35

second electron gain

Answer 35

it is always positive ,because repulsion increases after 1st electron

Question 36

factors affecting electron gain enthalpy

atomic size

Answer 36

down the group electron gain enthalpy decreases
across the periods increases
halogens have the highest value of electron gain enthalpy

Question 37

electropositivity

Answer 37

tendency to lose electron and attain positive ion
a more electropositive character means more metallic character
ACROSS THE PERIOD DECREASES
DOWN THE GROUP INCREASES

Question 38

analomous behavior

Answer 38

every 1st element of the every group is different from rest of the group 
smallest size 
highest IP 
highest value of EGE
highest electronegativity

Question 39

alkali metals

Answer 39

most reactive ,strongest reducing agent and have lowest IP

Question 40

halogens

Answer 40

most reactive ,strongest oxidizing agent anf have high IP

Question 41

Size of species

Answer 41

Size of species inversely proportional to nuclear charge

Question 42

Exception in electron gain enthalpy

Answer 42

In group 17 , cl > F because of F small size