Question:
Write the chemical formulae of the following. Also identify the ions present.
(a) Magnesium chloride
(b) Calcium oxide
(c) Copper nitrate
(d) Aluminium chloride
(e) Calcium carbonate.
Answer:
(a) Magnesium chloride: MgCl2 (ions present are: Mg2+, Cl1- )
(b) Calcium oxide: CaO (ions present are: Ca2+, O2- )
(c) Copper nitrate: Cu(NO3)2 (ions present are: Cu2+, NO31- )
(d) Aluminium chloride: AlCl3 (ions present are: Al3+, Cl1- )
(e) Calcium carbonate: CaCO3 (ions present are: Ca2+, CO32- )
Atoms and Molecules
Q 1.
Define 'formula mass' of a compound.
Q 2.
(i) State the law of constant proportions.
(ii) Show that water illustrates the law of constant proportions.
Q 3.
What is the chemical symbol for iron?
Q 4.
Write the chemical symbols of the following:
(i) Gold
(ii) Iron
(iii) Chlorine
(iv) Mercury
Q 5.
Name one element each which forms diatomic and tetra atomic molecule.
Q 6.
What is gram-atomic mass of an element?
Q 7.
Fill in the blanks:
The chemical symbol of mercury is _________.
Q 8.
How many atoms are there in 0.25 mole of hydrogen ?
Q 9.
Explain with example that law of conservation of mass is valid for chemical reactions.
Q 10.
Magnesium is two times heavier than C-12 atom, what shall be the mass of Mg atom in terms of atomic mass units? (Given mass of C-12 atom = 12u)
Q 11.
Define molecule. What are its important properties?
Q 12.
Fill in the blanks:
One mole of water contains ______________ molecules.
Q 13.
Give the names of the elements present in the following compounds.
(a) Quick lime
(b) Hydrogen bromide
(c) Baking powder
(d) Potassium sulphate.
Q 14.
What are ionic compounds?
Q 15.
Fill in the blanks:
The atomic mass of sodium is 23. The gram atomic mass of sodium is _________.
Q 16.
What is the molecular mass of a substance?
Q 17.
Which has more number of atoms, 100 grams of sodium or 100 grams of iron (given, atomic mass of Na = 23 u, Fe = 56 u)?
Q 18.
Find out number of atoms in 15 moles of He.
Q 19.
Who established the two important laws of chemical combinations?
Q 20.
Fill in the blanks:
Mass of 2 Hydrogen atoms is __________.
Q 21.
Calculate the formula unit masses of ZnO, Na
2O, K
2CO
3, given atomic masses of Zn = 65 u, Na = 23 u, K = 39 u, C = 12 u, and O = 16 u.
Q 22.
State whether the following statement is true or false :The symbol of element cobalt is CO.
Q 23.
Convert 12 g of oxygen gas into moles.
Q 24.
What is the mass of 5 moles of sodium carbonate (Na
) ?(Atomic masses : Na = 23 u ; C = 12 u ; O = 16 u)
Q 25.
Which postulate of Dalton’s atomic theory is the result of the law of conservation of mass?
Q 26.
Fill in the blanks:
The mass of 5 moles of ammonia (NH
3) is __________.
Q 27.
Based on type of substance, how molecules are classified?
Q 28.
What is valency of an element?
Q 29.
What is gram-molecular mass of a substance?
Q 30.
How many moles are there in 4.6 gms of Sodium(Na)?
Q 31.
Calculate the number of aluminium ions present in 0.051 g of aluminium oxide.
(
Hint: The mass of an ion is the same as that of an atom of the same element. Atomic mass of Al = 27 u)
Q 32.
Calculate the molecular masses of the following compounds :
(a) Methanol, CH
Q 33.
If one mole of nitrogen molecules weighs 28 g, calculate mass of one molecule of nitrogen in grams.
Q 34.
(a) What is meant by the 'molar mass'of a substance ? State the unit in which molar mass usually expressed.
(b) Calulate the molar masses of the following substances. Write the results with proper units
(1) Ozone molecule, O
Q 35.
What are the laws of chemical combinations?
Q 36.
State Law of constant proportions. Explain with an example.
Q 37.
Fill in the blanks:
The mass of 1 mole of a substance is called its _____________.
Q 38.
Why is it not possible to see an atom with naked eyes?
Q 39.
Name the international organization who approves names of elements.
Q 40.
Fill in the blanks:
According to law of definite proportions, in a chemical substance the elements are always present in __________ proportions by mass.
Q 41.
Fill in the blanks:
According to Dalton's atomic theory, atoms of different elements differ in ______, size and chemical properties.
Q 42.
Fill in the blanks:
The chemical symbol of flourine is ________.
Q 43.
Give four examples of diatomic molecules.
Q 44.
Give examples of triatomic molecules.
Q 45.
Calculate the molecular mass of chloroform (CHC1
Q 46.
Calculate the molecular mass of hydrogen bromide (HBr).
(Atomic masses: H=1; Br= 80 U)
Q 47.
An element X has a valency of 4 whereas another element Y has a valency of 1. What will be the formula of the compound formed between X and Y ?
Q 48.
How many atoms are present in one gram atomic mass of a substance ?
Q 49.
If 16 g of oxygen contains 1 mole of oxygen atoms, calculate the mass of one atom of oxygen.
Q 50.
Show by means of calculations that 5 moles of CO, and 5 moles of H
do not have the same mass. How much is the difference in their masses ?
