Question

essential aks review for test 3: bonding
bond properties

	ionic	polar	nonpolar
type of elements
what are electrons up to?
electronegativity difference
melting and boiling pts
dissolves in
states of matter
do they conduct electricity?
picture	image of ionic bond	image of polar bond	image of nonpolar bond
examples

Explanation:

This table is about bond properties in chemistry, which falls under the Natural Science discipline, specifically Chemistry. To fill it, we analyze each row for ionic, polar, and nonpolar bonds:

Type of elements:

• Ionic: Metal + non - metal (electron transfer between metal (loses e⁻) and non - metal (gains e⁻)).
• Polar: Non - metal + non - metal (unequal electron sharing due to electronegativity difference).
• Nonpolar: Non - metal + non - metal (equal electron sharing, same or similar electronegativity).

What are electrons up to?

• Ionic: Electrons are transferred from metal to non - metal, forming ions (cation: metal, anion: non - metal).
• Polar: Electrons are shared unequally; the more electronegative atom has a partial negative charge ($\delta^-$), the other a partial positive charge ($\delta^+$).
• Nonpolar: Electrons are shared equally between atoms.

Electronegativity difference:

• Ionic: $\geq 1.7$ (large difference, leading to electron transfer).
• Polar: $0.5 - 1.7$ (moderate difference, unequal sharing).
• Nonpolar: $< 0.5$ (small or no difference, equal sharing).

Melting and boiling pts:

• Ionic: High (strong ionic bonds, require much energy to break).
• Polar: Moderate (dipole - dipole forces, stronger than London dispersion in nonpolar, weaker than ionic).
• Nonpolar: Low (weak London dispersion forces, easy to break).

Dissolves in:

• Ionic: Polar solvents (e.g., water) - "like dissolves like" (ionic compounds are polar - charged ions interact with polar solvent molecules).
• Polar: Polar solvents (e.g., water, alcohol) - dipole - dipole interactions with solvent.
• Nonpolar: Nonpolar solvents (e.g., oil, hexane) - London dispersion forces with solvent.

States of matter:

• Ionic: Solid at room temp (strong ionic lattice structure).
• Polar: Liquid or gas (e.g., water is liquid, ammonia is gas) or solid (e.g., sugar), depending on molecular mass and intermolecular forces.
• Nonpolar: Gas (e.g., $O_2$, $N_2$) or liquid (e.g., oil) or solid (e.g., iodine), often low molecular mass ones are gases.

Do they conduct electricity?

• Ionic: Yes (when dissolved in water or molten, ions are free to move and carry charge). No in solid state (ions are locked in lattice).
• Polar: No (molecules, no free ions/electrons to conduct), unless ionized (e.g., acid in water).
• Nonpolar: No (molecular, no charge carriers).

Picture (as per given):

• Ionic: The first picture (large sphere - anion, small sphere - cation, with $-$ and $+$ signs).
• Polar: Middle picture (two spheres, $\delta^-$ and $\delta^+$ indicating unequal sharing).
• Nonpolar: Right picture (symmetrical, equal electron distribution).

Examples:

• Ionic: $\ce{NaCl}$ (Na - metal, Cl - non - metal), $\ce{MgO}$.
• Polar: $\ce{H_2O}$ (O more electronegative than H), $\ce{NH_3}$.
• Nonpolar: $\ce{O_2}$, $\ce{Cl_2}$, $\ce{CH_4}$ (in $\ce{CH_4}$, C - H bonds are nearly nonpolar, overall molecule is nonpolar).

Answer:

Bond Properties	Ionic	Polar	Nonpolar
What are electrons up to?	Electron transfer (metal $\to$ non - metal)	Unequal sharing (partial charges)	Equal sharing
Electronegativity difference	$\geq 1.7$	$0.5 - 1.7$	$< 0.5$
Melting and boiling pts	High	Moderate	Low
Dissolves in	Polar solvents (e.g., water)	Polar solvents (e.g., water)	Nonpolar solvents (e.g., oil)
States of matter	Solid (room temp)	Liquid/Gas/Solid	Gas/Liquid/Solid
Do they conduct electricity?	Yes (dissolved/molten), No (solid)	No (usually)	No
Picture	First (with $-$ and $+$)	Middle (with $\delta^-$/$\delta^+$)	Right (symmetrical)
Examples	$\ce{NaCl}$, $\ce{MgO}$	$\ce{H_2O}$, $\ce{NH_3}$	$\ce{O_2}$, $\ce{CH_4}$