📚Chemistry common questions about Periodic Table Trends
Instructions: Choose the single best answer for each question.
1. Which of the following properties generally INCREASES from left to right across a period in the periodic table?
a) Atomic radius
b) Ionization energy
c) Metallic character
d) Number of electron shells
Answer: b) Ionization energy
2. Which element has the highest electronegativity?
a) Fluorine (F)
b) Chlorine (Cl)
c) Francium (Fr)
d) Oxygen (O)
Answer: a) Fluorine (F)
3. As you move down a group in the periodic table, atomic radius generally:
a) Increases
b) Decreases
c) Remains constant
d) Shows no consistent trend
Answer: a) Increases
4. Which of these elements would be expected to have the largest ionic radius?
a) Li⁺
b) Na⁺
c) K⁺
d) Rb⁺
Answer: d) Rb⁺
5. Which of the following elements has the lowest first ionization energy?
a) Helium (He)
b) Sodium (Na)
c) Neon (Ne)
d) Argon (Ar)
Answer: b) Sodium (Na)
6. Electron affinity is best defined as the:
a) Energy required to remove an electron from an atom.
b) Tendency of an atom to attract electrons towards itself in a chemical bond.
c) Energy released or absorbed when an electron is added to a neutral atom.
d) Energy difference between the highest occupied and lowest unoccupied energy levels.
Answer: c) Energy released or absorbed when an electron is added to a neutral atom.
7. Which of these elements exhibits the most metallic character?
a) Carbon (C)
b) Silicon (Si)
c) Germanium (Ge)
d) Tin (Sn)
Answer: d) Tin (Sn)
8. Which of the following is a TRUE statement about electronegativity?
a) It is the same as electron affinity.
b) It only applies to ionic bonds.
c) It is a measure of an atom's ability to attract shared electrons in a covalent bond.
d) It increases down a group in the periodic table.
Answer: c) It is a measure of an atom's ability to attract shared electrons in a covalent bond.
9. Elements in the same group (vertical column) of the periodic table share similar chemical properties. This is primarily because they have the same:
a) Number of protons
b) Atomic mass
c) Number of valence electrons
d) Number of neutrons
Answer: c) Number of valence electrons
10. Which of the following correctly explains the general trend of ionization energy in the periodic table?
a) Increases across a period due to increasing nuclear charge.
b) Decreases down a group due to increasing shielding effect.
c) Both a and b
d) Neither a nor b
Answer: c) Both a and b
11. Elements with high electronegativity tend to form:
a) Positive ions (cations)
b) Negative ions (anions)
c) Metallic bonds
d) No ions at all
Answer: b) Negative ions (anions)
12. Which of the following statements about atomic radius is FALSE?
a) Cations are smaller than their parent atoms.
b) Anions are larger than their parent atoms.
c) Atomic radius increases as you move to the right across a period.
d) Atomic radius is influenced by the number of electron shells.
Answer: c) Atomic radius increases as you move to the right across a period.
13. Which periodic trend is responsible for the increasing reactivity of alkali metals (Group 1) as you move down the group?
a) Decreasing ionization energy
b) Increasing electronegativity
c) Increasing electron affinity
d) Decreasing atomic radius
Answer: a) Decreasing ionization energy
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Instructions: Choose the single best answer for each question.
1. Which of the following properties generally INCREASES from left to right across a period in the periodic table?
a) Atomic radius
b) Ionization energy
c) Metallic character
d) Number of electron shells
Answer: b) Ionization energy
2. Which element has the highest electronegativity?
a) Fluorine (F)
b) Chlorine (Cl)
c) Francium (Fr)
d) Oxygen (O)
Answer: a) Fluorine (F)
3. As you move down a group in the periodic table, atomic radius generally:
a) Increases
b) Decreases
c) Remains constant
d) Shows no consistent trend
Answer: a) Increases
4. Which of these elements would be expected to have the largest ionic radius?
a) Li⁺
b) Na⁺
c) K⁺
d) Rb⁺
Answer: d) Rb⁺
5. Which of the following elements has the lowest first ionization energy?
a) Helium (He)
b) Sodium (Na)
c) Neon (Ne)
d) Argon (Ar)
Answer: b) Sodium (Na)
6. Electron affinity is best defined as the:
a) Energy required to remove an electron from an atom.
b) Tendency of an atom to attract electrons towards itself in a chemical bond.
c) Energy released or absorbed when an electron is added to a neutral atom.
d) Energy difference between the highest occupied and lowest unoccupied energy levels.
Answer: c) Energy released or absorbed when an electron is added to a neutral atom.
7. Which of these elements exhibits the most metallic character?
a) Carbon (C)
b) Silicon (Si)
c) Germanium (Ge)
d) Tin (Sn)
Answer: d) Tin (Sn)
8. Which of the following is a TRUE statement about electronegativity?
a) It is the same as electron affinity.
b) It only applies to ionic bonds.
c) It is a measure of an atom's ability to attract shared electrons in a covalent bond.
d) It increases down a group in the periodic table.
Answer: c) It is a measure of an atom's ability to attract shared electrons in a covalent bond.
9. Elements in the same group (vertical column) of the periodic table share similar chemical properties. This is primarily because they have the same:
a) Number of protons
b) Atomic mass
c) Number of valence electrons
d) Number of neutrons
Answer: c) Number of valence electrons
10. Which of the following correctly explains the general trend of ionization energy in the periodic table?
a) Increases across a period due to increasing nuclear charge.
b) Decreases down a group due to increasing shielding effect.
c) Both a and b
d) Neither a nor b
Answer: c) Both a and b
11. Elements with high electronegativity tend to form:
a) Positive ions (cations)
b) Negative ions (anions)
c) Metallic bonds
d) No ions at all
Answer: b) Negative ions (anions)
12. Which of the following statements about atomic radius is FALSE?
a) Cations are smaller than their parent atoms.
b) Anions are larger than their parent atoms.
c) Atomic radius increases as you move to the right across a period.
d) Atomic radius is influenced by the number of electron shells.
Answer: c) Atomic radius increases as you move to the right across a period.
13. Which periodic trend is responsible for the increasing reactivity of alkali metals (Group 1) as you move down the group?
a) Decreasing ionization energy
b) Increasing electronegativity
c) Increasing electron affinity
d) Decreasing atomic radius
Answer: a) Decreasing ionization energy
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