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Elements and The Periodic Table Test

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Elements and The Periodic Table…

Chemistry 11 (SCH3U) Unit 1 – Matter, Chemical Trends, and Chemical Bonding Elements and The Periodic Table Test

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Question 1 of 30
1. Question
1 point(s)
Category: K/U
1. The atomic particle with the smallest mass is the
- a) electron
- b) proton
- c) neutron
- d) nucleus
- e) ion
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Question 2 of 30
2. Question
1 point(s)
Category: K/U
2. The atomic number of an element indicates the
- a) number of neutrons in the nucleus.
- b) number of protons in the nucleus.
- c) number of electrons in the nucleus.
- d) number of protons and neutrons in the nucleus.
- e) electron to proton ratio.
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Question 3 of 30
3. Question
1 point(s)
Category: K/U
3. The average atomic mass of Chlorine (35.452 u) is a good indication that
- a) Chlorine is a compound not an element.
- b) Chlorine is a mixture of isotopes.
- c) Chlorine nuclei contain fractions of a neutron.
- d) Chlorine consists of the molecule Cl2.
- e) Chlorine is radioactive.
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Question 4 of 30
4. Question
1 point(s)
Category: K/U
4. Which of the following elements requires the least amount of energy to remove an electron from an atom to form an ion?
- a) O
- b) He
- c) K
- d) H
- e) Fr
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Question 5 of 30
5. Question
1 point(s)
Category: K/U
5. Consider the equation A_(g) + energy –> A⁺ + e^–. The “energy” term in the equation represents
- a) electron affinity.
- b) heat of sublimation.
- c) atomic radii.
- d) ionization energy.
- e) sublimation energy.
Correct
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Question 6 of 30
6. Question
1 point(s)
Category: K/U
6. Electron affinity increases as you go from left to right on the periodic table because
- a) atomic radius decreases.
- b) ionization energy decreases.
- c) of the periodic law.
- d) all the above.
- e) none of the above.
Correct
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Question 7 of 30
7. Question
1 point(s)
Category: K/U
7. The first modern periodic table was developed by
- a) Dalton
- b) Democritus
- c) Thomson
- d) Mendeleev
- e) Chadwick
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Question 8 of 30
8. Question
1 point(s)
Category: K/U
8. Which of the following is NOT a metal?
- a) Li
- b) Al
- c) B
- d) Mg
- e) C
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Question 9 of 30
9. Question
1 point(s)
Category: K/U
9. Two atoms are isotopes if they have
- a) different atomic numbers.
- b) the same mass number, but different atomic numbers.
- c) the same number of protons and neutrons.
- d) the same number of electrons, but a different number of neutrons.
- e) the same atomic number, but a different mass number.
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Question 10 of 30
10. Question
1 point(s)
Category: K/U
10. The element found in the periodic table in Group 4 and Period 6 is
- a) hafnium, Hf.
- b) selenium, Se.
- c) gadolinium, Gd.
- d) chromium, Cr.
- e) aluminum, Al.
Correct
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Question 11 of 30
11. Question
1 point(s)
Category: K/U
11. According to the periodic law, chemical properties are repeated at regular intervals when
- a) elements are listed in order of their atomic radius.
- b) families of elements are listed in order.
- c) elements are listed in order of their date of discovery.
- d) elements are arranged in order of increasing atomic number.
- e) periods are arranged in order.
Correct
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Question 12 of 30
12. Question
1 point(s)
Category: K/U
12. A metalloid in Period 3 is
- a) scandium
- b) aluminum
- c) germanium
- d) phosphorus
- e) silicon
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Question 13 of 30
13. Question
1 point(s)
Category: K/U
13. The chemical family known as the halogens are the elements in Group
- a) 3
- b) 5
- c) 8
- d) 17
- e) 18
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Question 14 of 30
14. Question
1 point(s)
Category: K/U
14. When elements are arranged in order of increasing atomic mass, their chemical properties repeat at regular intervals. This statement is the definition of
- a) atomic mass.
- b) periodic law.
- c) limitations of the periodic table.
- d) law of definite proportions.
- e) law of conservation of mass.
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Question 15 of 30
15. Question
1 point(s)
Category: K/U
15. Isotopes with unstable nuclei are also referred to as
- a) nucleoisotopes.
- b) radioisotopes.
- c) isotopic radiation
- d) radiation.
- e) beta isotopes.
Correct
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Question 16 of 30
16. Question
1 point(s)
Category: T
16. The properties of elements repeat periodically if they are arranged by
- a) atomic mass.
- b) atomic charge.
- c) atomic number.
- d) number of neutrons.
- e) number of electrons.
Correct
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Question 17 of 30
17. Question
1 point(s)
Category: T
17. The mass listed for each element in the periodic table is
- a) the mass of all of the isotopes of the element combined.
- b) the mass of the average number of neutrons in all of the isotopes of the element.
- c) the average of the atomic masses of all of the isotopes of the element.
- d) the exact mass of the protons and neutrons in the most common isotope of the element.
- e) the weighted average of the atomic masses of all of the isotopes of the element.
Correct
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Question 18 of 30
18. Question
1 point(s)
Category: T
18. Why does atomic radius increase from top to bottom in a chemical family?
- a) Nuclear charge increases from top to bottom in a chemical family.
- b) Nuclear charge decreases from top to bottom in a chemical family.
- c) The number of energy levels increases from top to bottom in a chemical family.
- d) The number of energy levels decreases from top to bottom in a chemical family.
- e) The number of electrons decreases from top to bottom in a chemical family.
Correct
Incorrect
Question 19 of 30
19. Question
2 point(s)
Category: T
19. Why does atomic radius decrease from left to right in a period?
- a) Nuclear charge increases from left to right in a period.
- b) Nuclear charge decreases from left to right in a period.
- c) The number of energy levels increases from left to right in a period.
- d) The number of energy levels decreases from left to right in a period.
- e) The number of electrons decreases from left to right in a period.
Correct
Incorrect
Question 20 of 30
20. Question
2 point(s)
Category: T
20. Why does ionization energy increase from left to right in a period?
- a) Nuclear charge increases from left to right in a period.
- b) Nuclear charge decreases from left to right in a period.
- c) The number of energy levels increases from left to right in a period.
- d) The number of energy levels decreases from left to right in a period.
- e) The number of electrons decreases from left to right in a period.
Correct
Incorrect
Question 21 of 30
21. Question
2 point(s)
Category: T
21. Why does electron affinity increase from bottom to top in a chemical family?
- a) Nuclear charge increases from bottom to top in a chemical family.
- b) Nuclear charge decreases from bottom to top in a chemical family.
- c) The number of energy levels increases from bottom to top in a chemical family.
- d) The number of energy levels decreases from bottom to top in a chemical family.
- e) The number of electrons increases from bottom to top in a chemical family.
Correct
Incorrect
Question 22 of 30
22. Question
2 point(s)
Category: T
22. Why is it easier to remove an electron from potassium than it is to remove an electron from calcium?
- a) Potassium has a higher electron affinity.
- b) Potassium has a higher ionization energy.
- c) Potassium has a lower nuclear charge.
- d) Calcium has a lower electron affinity.
- e) Calcium is a metal, but potassium is not.
Correct
Incorrect
Question 23 of 30
23. Question
2 point(s)
Category: T
23. Which of the following is a practical use of radioisotopes?
- a) determining the age of old objects
- b) medical diagnosis
- c) production of electricity
- d) all of the above
- e) none of the above
Correct
Incorrect
Question 24 of 30
24. Question
2 point(s)
Category: T
24. Consider the equation X(g) + e^– –> X^– + energy. The “energy” term in the equation represents
- a) electronegativity
- b) electron affinity
- c) ionization energy
- d) nuclear charge
- e) none of the above
Correct
Incorrect
Question 25 of 30
25. Question
2 point(s)
Category: T
25. Elements A, B, C, and D (found in Groups 1–17) have atomic radii of 265 mm, 160 mm, 185 mm, and 175 mm, respectively. Which element will most likely have the highest ionization energy?
- a) A
- b) B
- c) C
- d) D
- e) Not enough information is given.
Correct
Incorrect
Question 26 of 30
26. Question
3 point(s)
Category: C
26. An aluminum atom contains 13 protons and 14 neutrons. What is the atomic number of Aluminum?
Correct
Incorrect
Question 27 of 30
27. Question
4 point(s)
Category: A
27. Examine the following graph and answer the questions below:
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a) What is the trend (from left to right) across a period?
b) What is the trend from top to bottom, down a group?
Correct
Incorrect
Question 28 of 30
28. Question
8 point(s)
Category: C
28. Draw the Bohr-Rutherford diagram for the Aluminum atom. You can either draw a complete B-R diagrams or a shorthand. If you cannot draw it here, scan your drawing and sending to your teacher or to admin@onstudy.ca
Correct
Incorrect
Question 29 of 30
29. Question
8 point(s)
Category: A
29. Different isotopes of the element X are shown in the table below.

Isotope Atomic mass Relative Abundance
X-28 27.98 m 92.23%
X-29 28.97 m 4.67%
X-30 29.97 m 3.10%

Determine the weighed average atomic mass of element X.
Correct
Incorrect
Question 30 of 30
30. Question
10 point(s)
Category: A
30. Complete the table below.
Isotope Mass number Atomic number Number of protons Number of neutrons Number of electrons
Beryllium-7 { } { } { } { } { }
{ } { } 29 { } { } { }
Correct
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