Chapter 7: Periodic Properties of the Elements

A set of flashcards covering key vocabulary and concepts related to the periodic properties of the elements, as discussed in the lecture.

Periodic Table

A tabular arrangement of chemical elements organized by their atomic number, electron configuration, and recurring chemical properties.

Electron Configuration

The distribution of electrons in an atom's orbitals, which dictates its chemical properties.

Henry Moseley

A scientist who rearranged the periodic table by atomic number, enhancing the organization and understanding of the elements.

Bonding Atomic Radius

The measure of the size of an atom, defined as one-half of the distance between two covalently bonded nuclei.

Cations

Positively charged ions that are smaller than their parent atoms due to the loss of electrons.

Anions

Negatively charged ions that are larger than their parent atoms due to the gain of electrons.

Isoelectronic Series

A group of ions that have the same number of electrons but different nuclear charges.

Ionization Energy

The energy required to remove an electron from an atom or ion in the gas phase.

First Ionization Energy (I1)

The energy needed to remove the first electron from a neutral atom in the gas phase.

Second Ionization Energy (I2)

The energy required to remove the second electron from a positively charged ion.

Periodic Trends

Patterns observed in the properties of elements as you move across a period or down a group on the periodic table.

Periodic Table

A tabular arrangement of chemical elements organized by their atomic number, electron configuration, and recurring chemical properties.

Electron Configuration

The distribution of electrons in an atom's orbitals, which dictates its chemical properties.

Henry Moseley

A scientist who rearranged the periodic table by atomic number, enhancing the organization and understanding of the elements.

Bonding Atomic Radius

The measure of the size of an atom, defined as one-half of the distance between two covalently bonded nuclei.

Cations

Positively charged ions that are smaller than their parent atoms due to the loss of electrons.

Anions

Negatively charged ions that are larger than their parent atoms due to the gain of electrons.

Isoelectronic Series

A group of ions that have the same number of electrons but different nuclear charges.

Ionization Energy

The energy required to remove an electron from an atom or ion in the gas phase.

First Ionization Energy (I1)

The energy needed to remove the first electron from a neutral atom in the gas phase.

Second Ionization Energy (I2)

The energy required to remove the second electron from a positively charged ion.

Periodic Trends

Patterns observed in the properties of elements as you move across a period or down a group on the periodic table.

Electronegativity

The measure of an atom's ability to attract electrons in a chemical bond.

Electron Affinity

The energy change that occurs when an electron is added to a neutral atom in the gas phase to form a negative ion.

Effective Nuclear Charge (Z_{\text{eff}})

The net positive charge experienced by an electron in a polyelectronic atom, considering both the actual nuclear charge and the shielding effect of inner-shell electrons.

Valence Electrons

The electrons in the outermost shell of an atom, which are primarily involved in chemical bonding.