Chemistry Ions and Bonding Quiz

Magnesium, a Group IIA element, loses two electrons when bonding with a nonmetal, forming a positive ion.

Using Lewis electron dot symbols, the final charge on the formed ion can be determined.

An anion has more electrons than its corresponding neutral atom.

The ammonia (NH3) molecule has two pairs of unshared electrons.

Potassium oxide (K₂O) is formed when potassium (K) transfers one electron to oxygen (O).

Based on Lewis electron dot symbols, Barium (Ba) is likely to form a +2 charge.

Phosphorus has 5 valence electrons in its Lewis electron dot symbol.

Ionic compounds conduct electricity in water because they dissociate into charged particles (ions).

In metallic bonding, valence electrons can move freely across the structure.

Ionic compounds like KCl have high melting points because of strong inter-ionic forces, while covalent compounds like CH4 have lower melting points.

Elements in Group IIA of the periodic table, like magnesium, tend to lose two electrons when they bond with nonmetals, forming positive ions with a +2 charge.

The Lewis dot structure of ammonia (NH3) shows nitrogen (N) with one lone pair of electrons and three shared pairs of electrons, each with one hydrogen (H) atom.

The final charge of an ion can be determined by counting the number of dots (representing valence electrons) in its Lewis electron dot symbol. Each dot represents one electron.

Potassium oxide (K2O) is formed when a potassium atom (K) loses one electron to an oxygen atom (O), resulting in K+ and O-2 ions.

An anion, like Cl-, has more electrons than its corresponding neutral atom (Cl). This extra electron gives the anion a negative charge.

Elements in Group IIA of the periodic table, like barium (Ba), have the highest tendency to lose two electrons and form a +2 charge.

Ionic compounds conduct electricity when dissolved in water because they dissociate into charged particles (ions) that can carry electrical current.

In metals, valence electrons are delocalized, meaning they're not bound to specific atoms and can move freely throughout the entire metal structure.

Dishwashing soap contains both polar and nonpolar molecules. The polar molecules attract water molecules, while the nonpolar molecules attract oil molecules, allowing the soap to remove grease and dirt.