State of Matter
CHEMISTRY - XI
Language of Chemistry
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What are molecules and compounds? Give two examples of radicals with
valency one two and three.
What are atomic number and atomic mass?
What is a molecular formulae? Write the molecular formula of following
compound.
(a) potassium chlorate
(b) sodium dichromate
(c) calcium chromate
(d) potassium permanganate
(e) magnesium sulphate
(f) ammonium phosphate
(g) aluminium sulphide
(h) strontium carbonate
(i) Sodium thiosulphate
39
What information can you obtain from the symbol 19 K?
How many electrons , protons and neutrons are present in the symbol
27
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What are gases? Give diagram to show the molecular arrangement of gases
Define the terms
(a) N.T.P.
(b) Absolute zero
(c) Diffusion
(d) Effusion
State Boyle’s law for gases and derive the relation for the effect of pressure
on volume at constant temperature. Draw the graph associated with this
law.
State and explain the Charle’s law.
Write the postulates of kinetic theory of gas?
What are ideal and real gases? What are the condition for the gas to deviate
from ideal behavior?
Write and expression for ideal gas equation. Derrive the ideal gas equation
based on Charle’s and Boyle’s law.
State and explain Dalton's law of partial pressure. Mention its one use.
+3
Al ?
Balance the following by hit and trial method:
(a) FeCl3 + H2 → FeCl2 + HCl
(b) Cu + H2SO4 → CuSO4 + SO2 + H2O
(c) AlN + H2O → Al(OH)3 + NH3
(d) Al4C3 + H2O → Al(OH)3 + CH4
Balance the following equations by partial equation methods.
(a) KMnO4 + HCl → KCl + MnCl2 + H2O + Cl2
(b) K2Cr2O7 + H2SO4 → K2SO4 + Cr2 (SO4)3 + H2O + O2
(c) Na2Cr2O7 + H2SO4 + H2S → Na2SO4 + Cr2 (SO4)3 + H2O + S
(d) Zn + HNO3 → Zn(NO3)2 + H2O + N2O
(e) Cu + H2SO4 → CuSO4 + H2O + SO2
(f) Cl2 + NaOH → NaCl + NaClO + H2O
(g) KI + H2SO4 → K2SO4 + H2O + SO2 + I2
What are radicals? Write the name of fifteen different radicals with their
valency and symbols.
Define atomic mass unit.
What is aqueous tension?
Atomic Structure
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What is an atom? what are subatomic particles? Name them. Make a table
to show the mass, charge and location of these sub-atomic particles in an
atom.
How was electron discovered?
With proper diagram show the Ruthordford gold foil experiment. Mention
the observations and the conclusion he made.
What observations led Ruthordford to make following conclusion.
i)
The atomic centre is positively charged.
ii) Most of the atomic space is hollow.
iii) The positive nucleus in an atom is very small.
Explain Rutherford atomic model and how did he explain the atomic
stability?
What are the drawbacks of Ruthordford’s atomic model?
What are the postulates of Bohr’s atomic model? How did it correct the
drawbacks of Ruthordford’s atomic model?
What are atomic spectra? How does Bohr’s atomic model explain the
origin of hydrogen spectrum?
What is hydrogen spectrum? Sketch and name various spectral series
observed in the atomic spectrum of hydrogen?
what are the limitations of Bohr’s atomic model?
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Which principle that goes against the concept of bohr’s fixed orbit? State
the principle?
Name the spectral series which appears in visual part of the
electromagnetic spectrum. How is such series originated?
Write short notes on Heisenberg's uncertainty principle and DeBroglie’s
equation.
What is an atomic orbital? What are shape of s and p-orbitals?
What is a quantum number? Mention the significance of four quantum
numbers.
What is principle quantum number and what is it’s significance?
What are azimuthal and magnetic quantum numbers? what do they signify?
State the Pauli exclusion principle, Hund's rule and Aufdau principle?
Give the electronic configuration of Cu(29) broming (Br = 35), chromium
(Cr = 24), Fe+2(26) and Cl – (17) is terms of orbitals.
An atomic orbital has n = 3 what are the possible value of l and m?
What are the values for n, l, m for 2px1 3s1 and 3d1 orbitals?
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Periodic Classification of Elements
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State Mendeleev's periodic law and modern periodic law.
Show your acquaintance with the following terms
(a) Periodic table
(b) Periodicity
(c) Atomic radius
(d) Electro negativity
(e) Electro affinity
(f) Ionization potential (or energy)
(g) Representative element
(h) Transition metals
(i) Noble or inert gases
Mention three advantages of Mendeleev's periodic table.
Write the important anomalies of Mendeleev's periodic table.
What are isotopes? Why was Mandeleev unable to explain the proper
position of the isotopes? How could the modern periodic table explains the
position of the isotopes.?
What are the features of modern periodic table and how can it correct the
anomalies of mandeleev’s periodic table?
What are iso-electronic species? Compare the size of F – and Na+ with neon
Which of the following have a larger size and why?
(i) Mg or Mg++
(ii) F or F –
(iii) K + or K
(ii) Cl – or Cl
–
+
(v) F , Na ,
(vi) Mg2+ or AI3+
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3+
(vii) Fe or Fe
(viii) N3 – or O2 –
18.
The Ca2+ and K+ have same number of electrons. Which ion would you
expect to have smaller radius? Why?
Why ionization energies of alkali metals decreases as the atomic number
increases?
Why is the ionization energy of Na greater than K?
Why is the ionization energy of oxygen less than that of nitrogen?
What is electron affinity? Compare the Electron affinity of (i) O & S (ii) F
& Cl with reasons.
What is ionization potential and what are the factors that affect the
ionization potential? Explain the trend of ionization potential across the
period and group.
Why do metal form cations where as nonmetals form anions?
What is periodicity? What causes periodicity? How does atomic radii vary
along the group and period in the periodic table?
Show your acquaintance with modern periodic table. Give the
characteristics of s, p,d and f block elements?
s- block, p-block and d-block have two, six and ten groups respectively.
Explain?
Why is the modern periodic table sometimes also called Bohr’s periodic
table?
NON-METALS
Hydrogen
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What are H, H+, H – and H2?
What are isotopes? Write all isotopes of hydrogen and mention any two
uses of these isotopes. Mention the isotope that contains no neutron.
Differentiate between ortho and para hydrogen.
Define nascent hydrogen. Write any two chemical reaction to show that
nascent hydrogen is more powerful reducing agent than molecular
hydrogen.
Mention an important use of each of the following.
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Most abundant isotopes of hydrogen
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Hydrogen gas
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Deuterium
Compare between nascent hydrogen and atomic hydrogen. Which is more
reactive and why?
What happens when zinc dust is added on hot potassium nitrate solution
made alkaline with potassium hydroxide?
Give two reaction to show that water contains hydrogen gas?
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When water is passed through red hot coke, a mixture of two gases is
produced. Name the gas and write the equation involves.
What is heavy water and mention important application of it?
Oxygen
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What are oxides? How are oxide classified?
Classify the following oxides with reasons:
Na2O, CaO, MgO, BaO, NO2, N2O5, CO2, SO2, SO3, ZnO, Al2O3, SnO,
H2O, H2O2, CO, NO, N2O, Na2O2, BaO2, FeO, Fe2O3, Pb3O4, I2O5 and P2O5
What are peroxides? Give one example of it. What is the oxidation number
of oxygen in peroxide.
Name the allotropes of oxygen and give an important use of it.
Name any two neutral oxide and give their molecular formula.
Mention an important use of the following.
Heavy water, ozone layer, allotrope of oxygen, amphoteric oxide, and
neutral oxide
Ozone
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Write the balanced chemical equation for the preparation of ozone from
oxygen? What do you mean by tailing of mercury?
Write the resonating structure of ozone.
What are CFCs? How do they deplete the ozone layer?
Write the action of ozone as (a) an oxidant (b) a bleaching agent and
(c) an additive
How is ozone layer being formed in stratosphere?
Write down the effects of ozone layer depletion.
What happens when:
(i) Silent electric discharge is passed through the pure and dry oxygen
(ii) mercury is exposed to ozonized atmosphere