Important Objectives for Chemistry
Paper XI
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1.
The decimal fractional part of
logarithm is called mantissa.
2.
At sea level and 0°C the atmospheric
pressure on each square inch of our body is 14.7
pounds.
3.
The oxidation potential of hydrogen
electrode is 0.00
volt.
4.
The number
of orbitals in the second energy level is 4.
5.
When the
value of Kc is very small, the product is unstable.
6.
Enzymes are proteins which catalyze a
chemical reaction in a living system.
7.
The value of
activation energy can be zero.
8.
Kp is
greater than Kc when reaction occurs with increase in volume of products.
9.
Isoelectric
ions have different number of protons but the same number of electrons.
10.
s-s sigma
bond is weaker than p-p sigma bond.
11.
In NH3
the nitrogen atom is sp3 hybridized.
12.
The reaction
of C + 2S ® CS2 is endothermic.
13.
Threshold energy is the
minimum amount of energy required for effective collision.
14.
Amorphous
boron is much
more reactive than crystalline boron.
15.
The rate of
reaction doubles for every 10°C rise in temperature.
16.
A solution,
which resists the changes in pH, is called a buffer solution.
17.
The pH of
lemon juice is likely to be 3.
18.
1dm3
of volume is equal to 1 liter.
19. Temperature-volume relationship is called Charles’ law.
20. X-rays are also called Roentgen rays.
21.
K+ is isoelectric with argon.
22.
The greater
the energy of activation, the less will be speed of reaction.
23.
Each carbon
atom in C2H2 is sp hybridized.
24.
Na+
has radius larger than that of Mg2+.
25.
Isotopes of
the same element have different atomic masses.
26.
In log
system the characteristic of 1000 is 3.
27.
The value of
order of reaction cannot be more than 3.
28.
The pH of 0.01M HCl solution is 2.
29.
The oxidation number of oxygen in H2O2
is –1
and in OF2 is +2.
30.
The volume of 1 gm of H2
gas at STP is 11.2 dm3.
31.
The oxidation number of ‘N’ in NO21¯
and NO31¯ are +3 and +5
respectively.
32.
Volume of 1 mole of chlorine gas at
STP is 22.4
dm3.
33.
Shorter the bond length, higher
will be bond energy.
34.
pH
+ pOH = 14.
35.
Oxidation takes place at anode
while reduction at cathode.
36.
Evaporation is a cooling process.
37. The blue colour of CuSO4 is due to the water of crystallization, [Cu(H2O)4]2+
39.
Number of electrons in Mg+2
is 10 and in O2¯
is 10.
40.
1s2, 2s2 2px1
is the electronic configuration of Boron.
41.
Cations have smaller radii than its
neutral atom.
42.
Anions are larger in size than its
parent atom.
43.
The shape of orbital for which l = 1 is dumb-bell.
44.
A solution which tends to resist
changes in pH is called Buffer.
45.
Shape of sp-hybrid orbital is Linear.
46.
Shape of sp2-hybrid orbital
is Trigonal.
47.
Shape of sp3-hybrid orbital
is Tetrahedral.
48.
There are 2 significant figures in 0.0021.
49.
The oxidation number of ‘Cr’ in K2Cr2O7
is +6.
50.
The substances undergoing decrease in
oxidation number is called Oxidizing Agent.
51.
The substances undergoing increase in
oxidation number is called Reducing Agent.
52.
Water rises in capillary tube due to Capillary
Action (Surface Tension).
53.
CO2 has zero
dipole moment due to its linear structure.
54.
The oxidation no. of Cl in HOCl is +1
and in HClO4 is +7.
55.
KMnO4 is an example of Oxidizing
Agent.
56.
1 M solution of KMnO4
contains 158
g/litre.
57.
1 N solution of KMnO4 contains
31.6
g/litre.
58.
The shape of H2O is Angular.
59.
The shape of CH4 is Tetrahedral.
60.
The shape of C2H4
is Trigonal.
61.
The shape of C2H2
is Linear.
62.
3.2 g of O2 gas at STP has
a volume 2.24
dm3.
63.
pH is the negative logarithm of Hydrogen Ion
Concentration, [H+].
64.
The oxidation number of ‘Mn’ in KMnO4,
K2MnO4, MnO2 and MnSO4 are +7,
+6,
+4 and +2 respectively.
65.
7.35 is the pH of human blood.
66.
35.5 g of Cl2 gas at STP
has a volume 11.2
dm3.
67.
1 N solution of oxalic acid contains 63 g/litre.
68.
The empirical formula of acetylene is
CH. Its molecular formula will be C2H2
if its molecular mass is 26.
69.
During
electrolytic conduction, cations are attracted towards cathode while anions are
attracted towards anode.
70.
A graph of volume with 1/P is straight
line.
71.
Reaction between an acid and alcohol
is called Esterification.
72.
Aqueous solution of Na2CO3
is basic
in nature.
73.
Aqueous solution of NH4Cl
is acidic in nature.
74.
The oxidation number of N in NCl3
is +3.
75.
The oxidation number of C in C2H6O
is –2.
76.
Universal indicator turns green
in neutral solution or water.
77.
Universal indicator turns yellow at pH 6.
78.
Universal indicator turns blue at pH 8.
79.
The amount of heat of neutralization
for strong acid and strong base is about 13700 calories.
80.
Fast reactions possess low
energy of activation.
81.
Slow reactions have high
energy of activation.
82.
Each orbital in an atom can be
completely described by Quantum Numbers.
83.
The addition of HCl to H2S
solution decreases
the ionization of H2S.
84.
A catalyst increases the velocity of a
reaction but decreases Ea.
85.
The reactions catalyzed by sunlight
are called Photochemical
Reactions.
86.
The e/m ratio of canal rays is the
highest when hydrogen
is taken in the discharge tube.
87.
The negative ion tends to expand with
the increase of negative charge on it.
88.
I.P. decreases in a group from
top to bottom.
89.
I.P. increases along each
period.
90.
Cesium is the most electropositive element.
91.
Fluorine is the most
electronegative element.
92.
Atomic
radii increase
down each group.
93.
Atomic
radii decrease
along each period.
94.
Dipole moment =
Charge (e) x distance between the
charges (d).
95.
1st
I.P. is always less than 2nd I.P.
96.
It
is easier to remove electron from Mg than
to Mg+.
97.
If
DE.N. between bonding atoms is greater than
1.7 than the bond between them will be ionic.
98.
If
DE.N. < 1.7, than the bond will be covalent.
99.
Water forms concave meniscus in glass
tube due to greater adhesive forces.
100.
Mercury forms convex meniscus in a glass tube due to greater cohesive
forces.
101.
Wetting liquids always form concave
meniscus.
102.
Non-wetting liquids always form convex
meniscus.
103.
Surface tension is inversely
proportional to the temperature.
104.
Viscosity of liquid decreases
with the rise of temperature (2% per degree).
105.
Viscosity of gases increases with the rise of temperature.
106.
Pmoist gas = Pdry gas + Pwater vapours.
107.
Partial pressure of a gas = Mole
fraction x Total pressure.
108.
Rate of diffusion
of a gas is inversely proportional to the square root of the density
(Molecular wt.) of the gas.
109.
Value of ‘R’ in dm3-atm
(Non-SI) is 0.0821.
110.
Value of ‘R’ in N-m or Joule (SI) is 8.3143.
111.
6.02
x 1023 molecules of N2
gas at STP has a volume 22.4 dm3.
112.
0°C
= 273.16 K.
113.
K
= °C + 273.
114.
The lowest possible temperature at
which all molecular motion ceases to exist is called Absolute Zero.
115.
1 atm
= 14.7
lb/inch2 (psi).
116.
1 atm
= 101325 (1.01325 x 105) N/m2.
117.
1 a.m.u. = 1.67 x 10¯24
g = 1.67 x 10¯27 kg.
118.
The value of ‘h’ in J.S. is 6.627 x 10¯34.
119.
120.
The radius of Bohr’s orbit is found
out to be 0.529
°A (0.0529 nm or 5.29 x 10-11 m).
121.
1°A
= 10¯10 m = 10¯8
cm.
122.
As the multiple bonds are shorter,
they have greater
bond energies than single bond.
123.
s-p sigma bond is stronger
than s-s sigma bonds.
124.
p-p sigma bond is stronger than s-p or s-s
sigma bonds.
125.
s-orbitals do not take part in
π-bond formation.
126.
The bond angle in CH4 is 109. 28°
while in C2H4 is 120°.
127.
Alpha rays have higher ionizing power than b
and g rays.
128.
Density, Pressure, M.P, B.P and
Refractive Index are Intensive Properties.
129.
Enthalpy, Internal Energy, Mass,
Volume and Mole are Extensive Properties.
130.
W is +ive when work is done on
system.
131.
W is –ive when work is done by
the system.
132.
The difference of
potential, create between a metal and solution of its salt is called Electrode
Potential of metal.
133.
Potential associated with oxidation is
called Oxidation
Potential.
134.
Potential associated with reduction is
called Reduction
Potential.
135.
Metals placed in the electro chemical
series above hydrogen act as anode (they are oxidized) while below hydrogen acts as cathode
(they are reduced).
136.
If the sign of electrode potential is positive,
then the reaction is spontaneous, and the electrode acts as anode whereas if the sign is negative then the electrode act
as cathode.
137.
The ratio F/NA represents
an electronic
charge.
138.
Ethyl acetate is an ester.
139.
I.P. of oxygen is less than that of nitrogen.
140.
Among Al3+, Mg2+
and Na1+ , Al3+ ion has the smallest
radius.
141.
Each carbon atom in C2H4
is sp2 hybridized.
142.
pH of 10-3 M NaOH solution
is 11
143.
The chemical formula of glucose is C6H12O6
144.
The formula of lime water is Ca(OH)2
145.
The standard temperature and pressure
are 273 K
and 1 atm.
146.
1cm3 of volume is equal to 1 ml.
147.
Pressure-volume relationship is called
Boyle’s
law.
148.
Roentgen rays are also called X-rays.
149.
Matter exists in 3
common physical states.
150.
CO2 has zero dipole moment
because of its linear structure.
151.
The reactions which proceed in one
direction are called irreversible reactions.
152.
The number of moles per dm3
is the molar
concentration.
153.
pH of buffer solution is constant.
154.
The greater the activation energy, the
less
will be the reaction rate.
155.
The value of principle quantum number (n)
cannot be zero.
156.
The value of azimuthal quantum number
cannot exceed than 3.
157.
Atomic number is the number of protons in an atom.
158.
The isotopes of the same element have
different number
of neutrons or physical properties.
159.
A catalyst speeds up a chemical
reaction by decreasing
activation energy.
160.
The value of azimuthal quantum number
cannot be more than three.
161.
Rate constant is dependent on temperature.
162.
When the value of n = 2, then values
of l are 0
and 1.
163.
Degree should not be used for kelvin
temperature scale.
164.
Alpha particles are helium
nuclei or doubly ionized helium atom.
165.
The bond length in CH≡CH is less
than that in CH2= CH2.
166.
Sigma bond is less reactive than pi
bond.
167.
Cooling is caused after evaporation.
168.
Elements form line spectrum.
169.
Mg2+ is isoelectronic with neon.
170.
Cl¯ is isoelectronic with argon.
171.
The pH range of phenolphthalein is 8.3-10.0
172.
The pH range of methyl orange is 2.9-4.6
173.
Electrode potential is a measure of electron losing or
gaining tendency of an electrode.
174.
The S.I. unit of R is J mol-1
K-1
175.
41.8 J is equal to 10
calories.
176.
1˚A corresponds to 10-9 nm.
177.
In BF3, boron is sp2
hybridized.
178.
In CO2, carbon is sp
hybridized.
179.
Lone pair-lone pair repulsion is greater than bond pair-bond pair repulsion.
180.
The molecular mass of Na2CO3
is 106
amu.
181.
64 g of SO2 contains 6.023x1023
number of molecules.
182.
The value of n cannot be zero.
183.
The value of l can
be zero.
184.
The average speed of the molecules in
a gas increases
with an increase in temperature.
185.
The universal gas constant R has the
dimensions of energy per mole per degree.
186.
Molecules of heavier gases diffuse slower.
187.
For an ideal gas, the value of
compressibility factor is 1.
188.
In molecular crystals, the constituent
particles are small molecules.
189. Graphite
is a covalent network crystal or macromolecular crystals.
190.
Liquids may be considered intermediate
between solids and gases.
191.
Small droplets of liquids assume spherical
shape due to surface tension.
192.
Hydrogen bonding in water is
responsible for its low vapour pressure at room temperature.
193.
Viscosity of liquids decreases
with a rise in temperature.
194.
The transition of electron in H atom
from 4th to 1st energy level emits a spectral line which
falls in Lyman
series.
195.
The azimuthal quantum number
specifies the shape of an orbital.
196.
The magnetic quantum number
signifies the spatial orientation of an orbital in space.
197. For
s orbitals, the orbital angular momentum is zero.
198.
h/π is the angular momentum in the 2nd shell of helium.
199. The
lowest energy state of an atom is called the ground state.
200.
The half-filled and completely filled
orbitals are more stable.
201.
CaCO3 exists in trigonal
and orthorhombic forms. This property is called polymorphism.
202.
NH4Cl is an acidic
salt.
203. As
the temperature of a liquid is increased, its viscosity decreases.
204. The
n+l value of 3d orbital is 5.
205.
The ionization energy of Be is greater than Li.
206.
The ionization energy of O is less
than N.
207.
The value of ionization potential decreases
with the increase of atomic size.
208. The
melting and boiling points of ionic compounds are high.
209.
SO2 molecule has planar
trigonal geometrical shape.
210. At
STP, the volume of 3.01 x 1023 molecules of H2 (or any)
gas is 11.2 dm3.
211. At
STP, the volume of 6.02 x 1024 molecules of H2 (or any)
gas is 224 dm3.
212. An
ideal gas obeys gas laws at All temperatures & pressures
213. Capillary
action of liquids is due to Surface
tension
214. Violet colour has the shortest wavelength in the visible spectrum of light (VIBGYOR).
215. Red colour has the shortest
wavelength in the visible spectrum of light (ROYGBIV)
216. Balmer series is produced when the electron jumps from the any higher orbit to 2nd
orbit
217. The
maximum number of electrons can be accommodated in f-orbital is 14.
218. The
maximum number of unpaired electrons can be accommodated in f-orbital is 7.
219. The
maximum number of electron pairs can be accommodated in f-orbital is 7.
220. The
maximum number of electrons can be accommodated in d-orbital is 10.
221. The
maximum number of unpaired electrons can be accommodated in d-orbital is 5.
222. The
maximum number of electron pairs can be accommodated in d-orbital is 5.
223. Among
hydrogen halide, HF has the highest percentage of ionic character
224. Among
hydrogen halide, HI has the least percentage of ionic character
225. (n+l)
value for 5d orbital is 7.
226. (n+l)
value for 4f orbital is 7.
227. (n+l)
value for 7s orbital is 7.
228. CO2 (CS2) has zero dipole
moment
229. 1
debye is equal to 3.335x10-30Cm
230. One
joule is equal to 0.239
cal.
231. Universal
indicator in acid gives Red
colour
232. Universal
indicator in base gives pink
colour
233. The
oxidation number of Mn in K2MnO4 is +6
234. The
rate of diffusion of CO2 is equal to that of C3H8
(propane).
235. The
S.I. unit of viscosity is N.s.m-2
235. The
cgs unit of viscosity is Poise
(Dyne.s.cm-2).
236. The
maximum number of electrons in a particular energy level is given by 2n2
237. The
maximum number of electrons in a particular sub-energy level is given by 2(2l+1).
238. The
energy of each quantum of radiation is directly proportional to its Frequency
239. The
energy of each quantum of radiation is directly proportional to its wave number
240. The
energy of each quantum of radiation is inversely proportional to its wave length.
241. g-rays are non-material in nature
242. The
potential energy of an electron can be denoted by ―Ze2/r.
243. Linear
molecules like CO2,
CS2 have the maximum bond angle (180).
244. Angular
molecules like H2O,
H2S have the least bond angle (104.5).
245. N2 has the greatest bond energy
246. The
dipole moment of Linear molecules like CO2, CS2 is
zero
247. For a reversible
reaction, if the concentrations of reactants are doubled, then the
equilibrium constant will Remain same
248. The number of bonds in C2H2
molecule is three σ and two p
249. Most of the radiations coming out from
pitch blende were Electrons
250. The melting points of those substances
which expand on melting increase when the pressure is increased
251. Dipole moment of CS2 is zero.
Hence the bond angle is 180°
252. Photochemical reactions, which proceed
only under the influence of light, are of the Zero order.
253. Glass is an amorphous solid or false solid or pseudo solid
254. The octet rule is not valid for this H2 molecule
255. Na+ and Mg2+ ions is isoelectronic
256. Violet has the shortest wavelength:
257. The SI unit of dipole moment is Coulomb- metre
258. 1 cal is equal to 0.239 J
259. Hydrogen bond is not a primary bond
260. Conduction in metals is due to the
movement of Electrons
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