Periodic Properties of the Elements

These flashcards cover the key concepts related to the periodic properties of elements, including atomic size, ionization energy, and trends in the periodic table.

Who independently developed concepts supporting the periodic table?

Dmitri Mendeleev and Lothar Meyer.

What property did Mendeleev use to organize his periodic table?

Atomic masses and chemical properties.

What is the effective nuclear charge equation?

Zeff = Z - S, where Z is the atomic number and S is the screening constant.

How does effective nuclear charge change across a period?

It increases across a period.

What is periodicity in the context of atomic properties?

The repetitive pattern of a property for elements based on atomic number.

What generally happens to atomic and ionic sizes moving down a group?

Atomic and ionic sizes increase down a group.

What is the definition of ionization energy?

The minimum energy required to remove an electron from a gaseous atom or ion.

How does ionization energy trend across a period?

Ionization energy generally increases across a period.

What effect do shelding and effective nuclear charge have on ionization energy?

Smaller atoms have higher ionization values due to higher effective nuclear charge.

What type of ion do metals typically form?

Cations.

What is a key characteristic of nonmetals?

Nonmetals typically form anions.

What characterizes the reactivity of alkaline earth metals compared to alkali metals?

Alkaline earth metals have higher densities and melting points, and their reactivity increases down the group.

What trend does electron affinity display as you move across a period?

Electron affinity generally increases across a period with notable exceptions.

What is the distinction between cations and anions in terms of size?

Cations are smaller than their parent atoms, while anions are larger.

Which group of elements contains the halogens?

Group 7A.

What states of matter can nonmetals be found in?

Nonmetals can be solid, liquid, or gas depending on the element.

Which group of elements is known for having very low reactivity?

Noble gases (Group 8A).

What happens to ionization energy as one moves down a group?

Ionization energy generally decreases down a group.

What is the smallest ion in an isoelectronic series?

The ion with the highest positive nuclear charge.