BL Ch 7 Periodic Properties

Multiple Choice

Who were the two scientists that independently concluded how elements should be grouped in the periodic table?

• Dmitri Mendeleev and Lothar Meyer

• Marie Curie and Ernest Rutherford

• John Dalton and J.J. Thomson

• Antoine Lavoisier and Robert Boyle

Open Ended

Why was the development of the periodic table significant in the field of chemistry?

Multiple Choice

Why do chemists credit Mendeleev for his work on the periodic table?

• He predicted missing elements and their properties using chemical properties.

• He discovered all elements.

• He organized elements by atomic number.

• He invented atomic theory.

Open Ended

How did the discovery of the atomic number change the organization of the periodic table?

Multiple Select

Which of the following properties are discussed as periodic properties in this chapter?

• Sizes of atoms and ions

• Ionization energy

• Electron affinity

• Boiling point

Multiple Choice

What is the formula for calculating effective nuclear charge (Z_eff)?

• Z_eff = Z - S

• Z_eff = S - Z

• Z_eff = Z + S

• Z_eff = Z / S

Open Ended

Based on the graph, explain how the effective nuclear charge changes as you move across a period in the periodic table.

Multiple Choice

Which of the following best defines the nonbonding atomic radius (van der Waals radius)?

• It is the distance between the nuclei of two bonded atoms.

• It is half of the shortest distance separating two nuclei during a collision of atoms.

• It is the distance from the nucleus to the outermost electron.

• It is the sum of the radii of two atoms.

Multiple Choice

How does the bonding atomic radius change as you move across a period and down a group in the periodic table?

• It increases across a period and decreases down a group.

• It decreases across a period and decreases down a group.

• It decreases across a period and increases down a group.

• It increases across a period and increases down a group.

Open Ended

Explain how ionic size is determined and what factors influence it.

Multiple Choice

Which element listed in the table experiences the largest increase in ionization energy between the removal of its last valence electron and the next electron?

• Na

• Mg

• Al

• Si

Open Ended

Explain how the trends in first ionization energy across a period and down a group are related to atomic structure.

Multiple Choice

Which of the following ions in the isoelectronic series O2−, F−, Na+, Mg2+, Al3+ has the smallest ionic radius?

• O2−

• F−

• Na+

• Al3+

Multiple Choice

Which of the following statements about ionization energy is correct?

• Smaller atoms have higher ionization energy values.

• Larger atoms have higher ionization energy values.

• Ionization energy does not depend on atomic size.

• Ionization energy is always the same for all elements.

Multiple Select

Select all statements that are true about ionization energy.

• Ionization energy is the minimum energy required to remove an electron from a gaseous atom or ion.

• The first ionization energy is required to remove the first electron.

• The higher the ionization energy, the easier it is to remove an electron.

• The second ionization energy is required to remove the second electron.

Multiple Select

Select all correct statements about electron configurations of ions.

• Cations lose electrons from the highest energy level.

• Anions gain electrons to fill ns2np6.

• Li+ loses a 2s electron.

• Fe2+ loses two 4s electrons.

Open Ended

Describe why electron affinity is typically negative for most elements and what this indicates about the process.

Multiple Choice

Which group in the periodic table is an exception to the general trend of increasing electron affinity across a period due to a full s sublevel?

• Group 2A

• Group 5A

• Group 8A

• Group 7A

Open Ended

Explain how the position of an element in the periodic table influences its metallic character.

Multiple Select

Which of the following statements about metals and nonmetals are correct?

• Metals tend to form cations.

• Nonmetals tend to form anions.

• Metals are found on the left side of the periodic table.

• Nonmetals have low electronegativity.

Open Ended

How has your understanding of the periodic properties of elements changed after this lesson?

Multiple Choice

What was the significant contribution of Dmitri Mendeleev and Lothar Meyer to the development of the periodic table?

• They discovered all the elements

• They independently concluded how elements should be grouped

• They invented the atomic model

• They created the first chemical reactions

Multiple Choice

What type of compound is most likely formed when a metal reacts with a nonmetal?

• Ionic

• Covalent

• Metallic

• Hydrogen bond

Open Ended

Describe two physical properties that distinguish nonmetals from metals.