Question

periodic trends review multiple choice

1. which statement best describes group 2 elements as they are considered in order from top to bottom of the periodic table? (a) the number of principal energy levels increases, and the number of valence electrons increases. (b) the number of principal energy levels increases, and the number of valence electrons remains the same. (c) the number of principal energy levels remains the same, and the number of valence electrons increases. (d) the number of principal energy levels remains the same, and the number of valence electrons decreases.
2. what is the total number of valence electrons in an atom of boron in the ground state? (a) 1 (b) 3 (c) 5 (d) 7
3. what is the total number of valence electrons in an atom of xenon, xe? (a) 0 (b) 2 (c) 8 (d) 18
4. the elements calcium and strontium have similar chemical properties because they both have the same (a) atomic number (b) mass number (c) number of valence electrons (d) number of completely filled sublevels
5. on the periodic table of the elements, all the elements within group 16 have the same number of (a) valence electrons (b) energy levels (c) protons (d) neutrons
6. an element with a partially filled d sublevel in the ground state is classified as (a) a halogen (b) a transition metal (c) an alkali earth metal (d) an alkali earth met
7. which electron - configuration represents a transition element? (a) 1s²2s²2p³ (b) ne3s² (c) ar4s²3d¹ (d) ar4s²3d¹⁰4p⁶
8. which element in period 5 of the periodic table is a transition element? (a) sr (b) sb (c) ag (d) xe
9. which of the following atoms has the largest atomic radius? (a) na (b) k (c) mg (d) ca
10. which noble gas has the highest first ionization energy? (a) radon (b) krypton (c) neon (d) helium
11. which sequence of elements is arranged in order of decreasing atomic radii? (a) al, si, p (b) li, na, k (c) cl, br, i (d) n, c, b
12. which list of elements from group 2 on the periodic table is arranged in order of increasing atomic radius? (a) be, mg, ca (b) ca, mg, be (c) ba, ra, sr (d) sr, ra, ba
13. as each successive element in group 13 of the periodic table is considered in order of increasing atomic number, the atomic radius (a) decreases (b) increases (c) remains the same
14. the strength of an atoms attraction for the electrons in a chemical bond is the atoms (a) electronegativity (b) ionization energy (c) heat of reaction (d) heat of formation
15. which properties are most common in nonmetals? (a) low ionization energy and low electronegativity (b) low ionization energy and high electronegativity (c) high ionization energy and low electronegativity (d) high ionization energy and high electronegativity
16. which group 17 element has the least attraction for electrons? (a) f (b) cl (c) br (d) i
17. which element in group 16 has the greatest tendency to gain electrons? (a) te (b) se (c) s (d) o
18. the group 17 element with the highest electronegativity is (a) fluorine (b) chlorine (c) bromine (d) iodine
19. as the elements of group 1 on the periodic table are considered in order of increasing atomic radius, the ionization energy of each successive element generally (a) decreases (b) increases (c) remains the same
20. the amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as (a) first ionization energy (b) activation energy (c) conductivity (d) electronegativity
21. which element is a member of the halogen family? (a) k (b) b (c) i (d) s
22. which of the following group 2 elements has the lowest first ionization energy? (a) be (b) mg (c) ca (d) ba

Explanation:

1. For question 1: As you go down Group 2 in the periodic table, the number of principal energy levels increases and the number of valence electrons remains 2.
2. For question 2: Boron is in Group 13, so it has 3 valence electrons.
3. For question 3: Xenon is a noble - gas in Group 18 and has 8 valence electrons.
4. For question 4: Elements in the same group have similar chemical properties because they have the same number of valence electrons. Calcium and strontium are in Group 2.
5. For question 5: All elements in Group 16 have 6 valence electrons.
6. For question 6: Transition metals have partially - filled d sub - levels in the ground state.
7. For question 7: A transition element has an electron configuration with partially - filled d orbitals. [Ar]4s²3d¹ is a transition - element configuration.
8. For question 8: Silver (Ag) is a transition element in Period 5.
9. For question 9: Atomic radius increases down a group and from right to left across a period. Potassium (K) has a larger atomic radius among the given options.
10. For question 10: Helium has the highest first ionization energy among noble gases due to its small size and high effective nuclear charge.
11. For question 11: Atomic radius decreases across a period. The order of decreasing atomic radius is Al > Si > P.
12. For question 12: Atomic radius increases down a group. The order of increasing atomic radius in Group 2 is Be < Mg < Ca.
13. For question 13: As you go down Group 13, the atomic radius increases with increasing atomic number.
14. For question 14: Electronegativity is the strength of an atom's attraction for the electrons in a chemical bond.
15. For question 15: Non - metals generally have high ionization energy and high electronegativity.
16. For question 16: Iodine (I) has the least attraction for electrons among Group 17 elements as electronegativity decreases down the group.
17. For question 17: Oxygen (O) has the greatest tendency to gain electrons in Group 16 as electronegativity decreases down the group.
18. For question 18: Fluorine has the highest electronegativity among Group 17 elements.
19. For question 19: As the elements of Group 1 are considered in order of increasing atomic radius, the ionization energy generally decreases.
20. For question 20: The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is the first ionization energy.
21. For question 21: Iodine (I) is a halogen.
22. For question 22: Barium (Ba) has the lowest first ionization energy among Group 2 elements as ionization energy decreases down the group.

Answer:

1. B
2. C
3. C
4. C
5. A
6. B
7. C
8. C
9. B
10. D
11. A
12. A
13. B
14. A
15. C
16. D
17. D
18. A
19. A
20. A
21. C
22. D