Water Basics and Importance

Water molecules are formed by two covalent bonds between oxygen and hydrogen atoms, with a bent shape.

A chemical bond formed by sharing electrons between atoms.

Relatively weak interactions between molecules.

Bonding within a molecule.

An important intermolecular force that occurs between water molecules.

Transitions between solid, liquid, and gaseous states of matter.

The ability of one substance to dissolve in another.

A measure of acidity or basicity of a solution.

Water is crucial for all life on Earth, covering 71% of the planet's surface.

Water exists naturally as solid (ice), liquid (water), and gas (water vapor).

Water found on the Earth's surface, like rivers, lakes, and streams.

Water found beneath the Earth's surface in aquifers.

Water with less than 1,000 milligrams per liter of dissolved solids (mostly salt).

Humans are mostly water (55-60%), varying by age and body composition (more fat, less water).

A molecule consisting of two hydrogen atoms and one oxygen atom (H₂O).

Most accessible freshwater is a small percentage of Earth's total water supply (around 0.3% of its 3% fresh water).

This is an attractive force that happens when polar molecules align so that the partially positive end of one molecule lines up close to the partially negative end of another.

Atoms that have a strong tendency to attract electrons towards themselves in a chemical bond.

Hydrogen bonding is unusually strong because when hydrogen is bonded to highly electronegative atoms, it becomes very slightly positive, making it strongly attracted to the negative end of other molecules.

Water is the only molecule on Earth that is naturally found in all three physical states: solid (ice), liquid (water), and gas (water vapor).

Hydrogen bonding is responsible for many of water's unique properties, such as its high boiling point, surface tension, and ability to dissolve many substances.

Hydrogen bonds are the primary force responsible for water's cohesive and adhesive properties, affecting its role in biological processes and environmental phenomena.

Hydrogen bonding is the key to many of water's amazing properties, including its high surface tension – think of how water bugs can walk on water – and its ability to dissolve many substances – like sugar in your coffee.

The individual water molecules (H2O) remain intact, meaning the atoms within the molecule don't change. Only the arrangement and interactions between molecules change.

The intermolecular forces, the attractions between water molecules, change. These forces dictate the arrangement and movement of molecules, leading to different physical states.

Water is polar because the oxygen atom attracts electrons more strongly than the hydrogen atoms, creating a partial negative charge on the oxygen and a partial positive charge on the hydrogens.

It represents a 'partial negative' charge. This means the atom has a slightly negative charge due to an imbalance in electron sharing.

It represents a 'partial positive' charge. This means the atom has a slightly positive charge due to an imbalance in electron sharing.

The attraction between polar molecules, where the partially positive end of one molecule is attracted to the partially negative end of another molecule.

It causes water molecules to align themselves so that the positive ends of one molecule are near the negative ends of another molecule, leading to strong interactions.

It is responsible for many of water's unique properties, such as its high boiling point, surface tension, and ability to dissolve many substances.