General, Organic, and Biochemistry: Chapter 2 - The Structure of the Atom and the Periodic Table

This set of flashcards covers key concepts from Chapter 2 on the structure of the atom and the periodic table, including atomic theory, properties of subatomic particles, isotopes, and trends in the periodic table.

What is the definition of an atom?

The basic structural unit of an element and the smallest unit that retains the chemical properties of that element.

What are the three primary particles that compose an atom?

Protons, neutrons, and electrons.

What is the charge and location of electrons in an atom?

Electrons are negatively charged particles located outside of the nucleus.

What is the nucleus and what does it contain?

The nucleus is a small, dense, positively charged region in the center of the atom that contains protons and neutrons.

What relationship defines a neutral atom?

A neutral atom has the same number of protons and electrons.

Define isotopes.

Isotopes are atoms of the same element having different masses, containing the same number of protons but different numbers of neutrons.

What is the atomic number and what does it represent?

The atomic number (Z) is the number of protons in the atom.

What is the mass number and how is it calculated?

The mass number (A) is the sum of the number of protons and neutrons.

What does Dalton's Atomic Theory state about matter?

All matter consists of tiny particles called atoms and cannot be created, divided, destroyed, or converted to other types.

What was revealed by Rutherford's Gold Foil Experiment?

Most of the atom is empty space and the majority of the mass is located in a small, dense region, the nucleus.

What does the term 'periodic law' refer to?

The physical and chemical properties of the elements are periodic functions of their atomic numbers.

What is the Octet Rule?

Elements typically react to attain the electron configuration of the nearest noble gas, aiming for a full complement of valence electrons.

Define cations and anions.

Cations are positively charged ions formed by the loss of electrons, while anions are negatively charged ions formed by the gain of electrons.

What are the main properties of metals?

High thermal and electrical conductivities, high malleability and ductility, and metallic luster.

What are the properties of nonmetals?

Brittle, often powdery solids or gases, with properties generally opposite to those of metals.

What is ionization energy?

The energy required to remove an electron from an isolated atom.

What does electron affinity signify?

The energy released when a single electron is added to an isolated atom, indicating the ease of anion formation.