Concept 3 Periodic Trends Unit 3

Explain how Coulomb's law is related to the periodic trends observed in the periodic table.

• Coulomb's law explains the attraction between protons and neutrons, which affects periodic trends.

• Coulomb's law describes the force between charged particles, influencing trends like atomic radii and ionization energy.

• Coulomb's law is unrelated to periodic trends as it only applies to gravitational forces.

• Coulomb's law only affects the trends of transition metals.

Which of the following best describes the trend in atomic radii across a period in the periodic table?

• Atomic radii increase as you move from left to right across a period.

• Atomic radii decrease as you move from left to right across a period.

• Atomic radii remain constant across a period.

• Atomic radii increase and then decrease across a period.

Analyze the trend in reactivity for alkali metals as you move down the group. What is the reason for this trend?

• Reactivity decreases due to increased ionization energy.

• Reactivity increases due to decreased ionization energy.

• Reactivity remains constant due to similar atomic structure.

• Reactivity decreases due to increased electronegativity.

Which of the following best explains the trend in electronegativity across a period?

• Electronegativity decreases as you move from left to right across a period.

• Electronegativity increases as you move from left to right across a period.

• Electronegativity remains constant across a period.

• Electronegativity increases and then decreases across a period.

Describe the trend in ionization energy as you move down a group in the periodic table.

• Ionization energy increases as you move down a group.

• Ionization energy decreases as you move down a group.

• Ionization energy remains constant down a group.

• Ionization energy increases and then decreases down a group.

Explain how the shielding effect influences the periodic trend of atomic radii.

• The shielding effect increases atomic radii by reducing the effective nuclear charge.

• The shielding effect decreases atomic radii by increasing the effective nuclear charge.

• The shielding effect has no influence on atomic radii.

• The shielding effect only affects transition metals.

Predict the type of bond that would form between sodium (Na) and chlorine (Cl) based on their electronegativity difference.

• Covalent bond

• Ionic bond

• Metallic bond

• Hydrogen bond

Calculate the difference in electronegativity between hydrogen (2.1) and oxygen (3.5) and predict the type of bond that would form.

• 1.4, covalent bond

• 1.4, ionic bond

• 1.4, polar covalent bond

• 1.4, metallic bond

Identify the oxidation number for elements in Group 1 of the periodic table.

• +1

• +2

• +3

• 0

Which of the following elements is most likely to form a cation?

• Fluorine

• Sodium

• Oxygen

• Chlorine