Molecular and Ionic Bonding

Malleability due to mobile valence electron clouds surrounding metal cations.

Flexibility from weak van der Waals forces between neutral molecules in a covalent network.

High melting points due to strong electrostatic forces between ions in a network solid.

Brittleness caused by rigid ion arrangements susceptible to fracture under stress.

Covalent bond

Metallic bond

Ionic bond

Hydrogen bond

Alloying reduces hardness since additional elements disrupt cohesive forces between metal ions decreasing overall structural integrity.

Alloying has no effect on hardness since only temperature changes impact atomic vibrations which determine material hardness.

Alloying causes fluctuation in hardness depending on whether added elements are metals or nonmetals without predictable trends.

Alloying typically increases hardness due to distortion of regular crystal lattice structures making dislocation movement more difficult.

Positive and negative ions held together by electrostatic attractions

An array of cations surrounded by a 'sea' of valence electrons

Atoms or molecules connected via LDFs, dipole-dipole, or hydrogen bonds

A network of covalent bonds between atoms

Ductility increases while hardness decreases because alloying makes materials more malleable but softer.

Both ductility and hardness increase since additional elements act as reinforcement within the metallic structure, enhancing its properties uniformly.

Both ductility and hardness decrease as additional elements create defects within the metal lattice structure making it weaker overall.

Ductility decreases while hardness increases with added alloying elements due to structural disruptions.

The equilibrium position will become indeterminate.

The equilibrium will shift to favor reactant formation.

The equilibrium will continue to favor product formation.

The equilibrium will remain unchanged.

It describes a 'sea' of delocalized electrons that move freely and carry charge through the wire.

It suggests that copper atoms share electrons equally, promoting easy flow of current.

It indicates that copper ions are mobile and can flow as electric current in solid state.

It posits that stationary copper nuclei create a path for electrons by direct transmission between them.

Smaller size variation tends to enhance thermal conductivity as smaller atoms encourage uniform energy distribution.

Increasing size discrepancy generally leads to greater hardness and brittleness owing to the stresses created within the crystal structure.

Larger differences in atomic radius may lead to reduced overall weight as larger constituents take up more space.

Varying atomic sizes can result in increased transparency as larger gaps produce fewer scattering points for light.

It reduces electron mobility leading directly to decreased electrical resistivity and increased luster.

It induces phase changes that make metals more malleable at low temperatures without affecting toughness.

It causes recrystallization that leads to softening without altering electrical conductivity significantly.

It increases dislocation density which enhances strength but decreases ductility.

Solution

Polymer

Compound

Alloy