Introduction to Atomic Structure and Bonding

These flashcards cover key concepts related to atomic structure, bonding, and the periodic table as discussed in the lecture.

Atomic Number

The number of protons in the nucleus of an atom, which determines the element's identity.

Mass Number

The total number of protons and neutrons in an atomic nucleus.

Protons

Positively charged particles found in the nucleus of an atom.

Neutrons

Neutral particles found in the nucleus of an atom.

Electrons

Negatively charged particles that orbit the nucleus of an atom.

Stable Atom

An atom with an equal number of protons and electrons.

Chemical Bond

The attraction between atoms that leads to the formation of molecules.

Ionic Bond

A type of bond that occurs when one atom steals electrons from another atom.

Covalent Bond

A type of bond formed when two atoms share electrons.

Energy Level

The specific distance from the nucleus where electrons are likely to be found.

Valence Electrons

Electrons in the outermost shell that determine an atom's bonding behavior.

pH Scale

A scale used to specify the acidity or basicity of a solution.

Chemical Reaction Indicators

Changes such as temperature, color, gas bubbles, or formation of a solid that indicate a chemical reaction has occurred.

Sodium Atom (Na)

An atom with 11 protons and 11 electrons.

Sodium Ion (Na+)

A sodium atom that has lost one electron, resulting in 11 protons and 10 electrons.

Chlorine Atom (Cl)

An atom with 17 protons and 17 electrons.

Chloride Ion (Cl-)

A chlorine atom that has gained one electron, resulting in 17 protons and 18 electrons.

Sodium Chloride (NaCl)

A molecule composed of one sodium ion and one chloride ion.

Calcium Atom (Ca)

An atom with 20 protons and 20 electrons.

Oxygen Atom (O)

An atom with 8 protons and 8 electrons.

Oxide Ion (O2-)

An oxygen atom that has gained two electrons, resulting in 8 protons and 10 electrons.

Double Bond

A type of covalent bond where two pairs of electrons are shared between two atoms.

Organic Molecules

Molecules primarily made of carbon atoms bonded to hydrogen and other elements.

Hydrogen Bonding Capacity

1; hydrogen typically forms one covalent bond.

Nitrogen Bonding Capacity

3; nitrogen can form three covalent bonds.

Carbon Bonding Capacity

4; carbon can form single or double covalent bonds.

Atom

The smallest unit of matter that retains the properties of an element.

Subatomic Particles

Protons, neutrons, and electrons, which make up an atom.

Nucleus

The central part of an atom, containing protons and neutrons.

Electron Configuration

The arrangement of electrons in an atom's energy levels.

Electron Weight

Considered negligible compared to protons and neutrons in mass calculations.

Mass of Proton/Neutron

Approximately equal in weight and significantly greater than that of an electron.

Element

A substance made of only one type of atom.

Periodic Table

A chart that organizes all known elements by increasing atomic number.

Manmade Elements

Elements that are artificially created and not found in nature.

Natural Elements

Elements that occur naturally in the environment.

Ion

An atom that has gained or lost one or more electrons, resulting in a charge.

Sodium Chloride Properties

Composed of Na+ and Cl- ions, showing ionic bonding characteristics.

Bonding Behavior

Determined by the number of valence electrons available in an atom.

Electronic Configuration for Carbon

2 electrons in the first energy level, 4 in the second.

Hydrogen Atom Composition

Has 1 proton and 1 electron.

Helium Atom Composition

Has 2 protons and 2 electrons.

Periodic Table Arrangement

Elements are organized from simplest to most complex.

Scientific Explanation of Atoms

Atoms cannot be broken down without losing their unique properties.

Key to Chemical Properties

Based on the number and arrangement of subatomic particles.