Atomic Interaction Forces Quiz

Different types of orbitals within an energy level of an atom, where electrons reside.

Different types of electron orbitals, each with a unique shape and electron capacity.

Distinct energy states for electrons in an atom, denoted by integers (n=1, 2, 3...).

Spherical orbital shape, holding a maximum of 2 electrons.

Dumbbell-shaped orbital, holding up to 6 electrons.

More complex orbital shape (clover-like), holding up to 10 electrons.

Electrons closer to the nucleus have lower energy; farther electrons have higher.

Energy levels are divided into subshells (s, p, d, f) according to the electron's energy and position.

Forces that hold atoms together in a solid.

Attractive force between positive and negative charges.

Combination of attractive and repulsive forces between atoms.

Force pushing atoms apart at short distances.

Force pulling atoms together at larger distances.

Distance where attractive and repulsive forces balance.

Energy associated with the forces holding atoms together.

Atoms attract due to the coulombic force between positive and negative charges.

The forces of attraction and repulsion between atoms.

The force that pulls atoms together.

The force that pushes atoms apart.

The overall force on an atom, calculated by combining attractive and repulsive forces.

The separation between atoms where the net force is zero.

Energy associated with the interaction between atoms.

Energy associated with the attractive force between atoms, decreases as distance gets smaller.

Energy associated with the repulsive force between atoms, increases as distance gets smaller.

Atoms attract when stretched and repel when compressed. The net force is the sum of attractive and repulsive forces.

Transfer of valence electrons between metallic and non-metallic elements, creating oppositely charged ions attracted to each other.

Strong chemical bonds between atoms including ionic, covalent, and metallic.

Electrostatic forces of attraction between oppositely charged ions.

Resultant force from the combination of attractive and repulsive forces in bonding.

Distance between two atoms where attractive and repulsive forces are balanced, resulting in minimum potential energy.

Energy required to separate the atoms to an infinite distance.

Sharing of valence electrons between atoms, often directional

Weak bonds between atoms or molecules, typically 10 kJ/mol.

Forces arising from temporary dipoles, causing weak attraction between molecules.

A molecule with separated positive and negative charges.

Energy required to break a bond between atoms or molecules.

Strong bonds, e.g., ionic, covalent, and metallic, holding atoms together in solids.

Electron transfer creating charged ions and attraction between opposite charges.

Electron sharing between atoms.

Valence electrons forming a 'sea of electrons' around metal ions.

Atoms transfer electrons to achieve stable electron configurations, creating oppositely charged ions that attract.

Atoms share electrons to achieve stable electron configurations. Each atom contributes at least one electron.

Covalent bonds have specific directions, limiting possible atomic arrangements.

Valence electrons are shared throughout the metal, forming a "sea" of electrons that surround positively charged ions.

Metals have 1,2, or 3 valence electrons that are mobile.

The remaining non-valence electrons and nuclei form positively charged particles in metals.

A model of metallic bonding in which valence electrons are considered to move freely through the metal.

The electrostatic attraction between positively charged ions and the surrounding 'sea' of free-moving electrons in a metal.