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WorksheetsMatter and Atomic Structure
Total questions: 35
Worksheet time: 18mins
How many protons (p), neutron (n) and electrons(e) are present in the Aurum isotope?
79 p 79 e 79 n
79 p 118 e 79 n
79 p 79 e 118 n
118 p 79 e 79 n
Determine the molar mass of Cu(NO3)2
186.7 grams per mol
186.7 grams
187.6 grams
187.6 grams per mol
One mole of H2SO4 has a mass of ?
98.1 grams
12 grams
90 grams
96.1 grams
The following statement is false about molar mass of an element except ?
mass of one mole of an element compared to 12 grams of one atom of carbon-12.
mass of one mole of an element compared to 1/12 mass of an atom carbon with mass of 12 grams.
mass of one mole of a molecule compared to 12 grams of one atom of carbon-12.
mass of one mole of a molecule compared to 1/12 mass of an atom carbon with mass of 12 grams.
Define empirical formula
A chemical formula that shows the actual number of all atoms in a molecule.
A chemical formula that shows the smallest ratio of all elements in a compound.
A chemical formula that shows the highest ratio of all elements in a compound.
A chemical formula that shows the actual number of all elements in a compound.
Calculate the relative molecular mass of MgSO4.7H2O ?
246.1 g/mol
120.1 g/mol
246.1
120.1
Determine x in the following hydrated compound formula, CuSO4. xH2O given that the relative molecular mass is 249.7.
5
6
7
8
_____________ is defined as number of solute dissolved per litre of solution.
Molality
Molarity
Molal
Mole fraction
If there is 12 litre of 0.25 M HCl solution, calculate the number of moles present.
0.3 moles
0.03 moles
3.00 moles
0.0003 moles
Determine the molality of a 0.04 moles of NaOH solution in 250 grams of water.
0.16 m
0.016 m
1.6 m
0.0016 m
Which of the following is true about dilution
the final volume is smaller than the initial volume.
the number of moles of solute present is the same.
the number of moles of solute will increase after dilution.
the volume of solution remains the same.
What is the molarity of HNO3 solution made by diluting 250.0 mL of a 1.60 M solution to final volume of 400.0 mL ?
1.20 M
1.00 M
0.20 M
0.16 M
Which of the following statement is true about limiting reactant ?
has smaller molar mass
is consumed mostly
has smaller coefficient
is consumed completely
The excess reactant in a chemical reaction is the one that
is consumed completely.
limits the amount of products formed.
is not consumed completely.
has smaller amount than limiting reactant.
Which of the following is not Bohr’ s atomic postulate ?
Electron moves in circular orbit around the nucleus.
Electrons have both wave and particle properties.
Energy of an electron is quantised.
Electron is unstable at excited state.
Electrons has a fixed allowed orbit. This means that the energy of an electron is __________
quantised
dequantised
emitted
released as photon
What happens to an electron at excited state ?
It gains energy and promoted to higher energy level.
it falls back to ground state and maintains its energy.
it is stable and remains at the excited state.
it falls back and release energy in the form of photon.
Calculate the energy of the electron in the diagram.
1.36 x 10-19 J
1.36 x 10-19 kJ
— 1.36 x 10-19 J
— 1.36 x 10-19 kJ
When electron falls back to ground state n = 2, the spectral lines formed are called ____________.
Lyman series
Balmer series
Brackett series
Pfund series
The following emission series are found in the infrared region except for ?
Pfund series
Paschen series
Lyman series
Brackett series
Which line has the longest wavelength?
Line E
Line C
Line D
Line A
Which line has the greatest energy and frequency ?
Line A
Line C
Line D
Line E
Given that the spectral lines is in Paschen series, how line B in the line spectrum is formed ?
transition of an electron from n = 5 to n = 3
transition of an electron from n = 3 to n = 5
transition of an electron from n = 7 to n = 3
transition of an electron from n = 3 to n = 7
Which transition below gives rise to the second line in Lyman series
n = 3 to n = 2
n = 3 to n = 1
n = 4 to n = 1
n = 3 to n = 2
One of the Bohr’s atomic postulate suggests that electron moves in a circular orbit around the nucleus and its energy is quantised. Which principle rejects this idea?
Pauli Exclusion Principle
Heisenberg’s Uncertainty Principle
Aufbau Principle
Hund’s Rule
Dual nature of electrons are theory proposed by ?
Neils Bohr
Wolfgang Pauli
Louis de Broglie
Werner Heisenberg
Which of the following is related to Heisenberg’s Uncertainty Principle ?
the more accurately we know about a momentum of an object, the more accurately we know about its location.
the more accurately we know about a momentum of an object, the more accurately we know about its mass.
the more accurately we know about a momentum of an object, the less accurately we know about its mass.
the more accurately we know about a momentum of an object, the less accurately we know about its location.
The following properties are related to angular momentum quantum number except ?
orientation in space
energy sublevel
orbital shape
energy level shape
the possible orbitals for n = 3 are ?
s orbital only
s and p orbitals only
s, p and d orbitals
s, p, d and f orbitals
Which of the following best describes Aufbau Principle
Electrons are filled from the lowest energy orbital to the highest energy orbitals
Electrons are filled from the highest n orbital to the lowest energy orbitals
Electrons are filled from the lowest n orbital to the highest energy orbitals
Electrons are filled from the highest energy orbital to the lowest energy orbitals
“When filling electrons in the degenerate orbitals, the electrons are filled singly first before it is paired.”
This statement is related to ?
Bohr’s Atomic Postulate
de Broglie’s Postulate
Hund’s Rule
Aufbau Principle
Which rule does the electrons in the diagram violate ?
Aufbau Principle
Heisenberg’s Uncertainty Principle
Pauli Exclusion Principle
Hund’s Rule
Which of the following best describes Hund’s Rule ?
when atomic orbitals of equal energy are filled, the ground state electronic configurations is that with the most paired electrons.
when degenerate orbitals are filled, the ground state electronic configurations is that with the most paired electrons.
when degenerate orbitals are filled, the ground state electronic configurations is that with the most unpaired electrons.
when atomic orbitals of equal energy are filled, the ground state electronic configurations is that with the most doubled up electrons.
“No two electrons in an atom can have the same four quantum numbers.”
This is the definition for
Bohr’s theory
Heisenberg’s Uncertainty Principle
Hund’s Rule
Pauli Exclusion Principle
Ne has 10 electrons. How many electrons are there in Na+ ion?
10
11
12
13
