The boiling point is the temperature at which a liquid turns into vapor.

The boiling point is defined as the temperature at which a liquid's vapor pressure equals the external pressure.

The melting point is the temperature at which a solid becomes a liquid.

The transition from a gas to a liquid is called condensation.

Sublimation is the process where a solid transitions directly to a gas without becoming a liquid.

Evaporation is the process of a liquid turning into gas below its boiling point.

Evaporation is the process where liquid turns into gas.

Sublimation is the process where a solid turns directly into a gas.

The term 'adsorption capacity' refers to the amount of solute that can be adsorbed per unit mass of adsorbent.

10 g of Na = 0.434 moles. 2Na + H2SO4 → Na2SO4 + H2. 0.434 moles of Na2SO4 = 0.434 * 142 g = 61.6 g.

23 g of Na = 1 mole. 1 mole of Na produces 1 mole of NaCl = 58.5 g.

23 g of Na = 1 mole. 1 mole of Na produces 1 mole of NaCl = 58.5 g.

1 mole of CO2 contains 1 carbon atom and 2 oxygen atoms, totaling 3 atoms.

C2H5OH has 2 carbon, 6 hydrogen, and 1 oxygen atom, totaling 7 atoms.

C4H10 has 4 carbon atoms and 10 hydrogen atoms, totaling 14 atoms.

The total number of electrons is 36 (from Kr) + 2 (from 5s2) + 10 (from 4d10) + 5 (from 5p5) = 53.

The decomposition reaction is CaCO3 → CaO + CO2. This produces 1 mole of CaO and 1 mole of CO2, totaling 2 moles of gas.

The decomposition of CaCO3 produces CaO and CO2: CaCO3 → CaO + CO2. This results in 1 mole of gas (CO2) being produced.

The n=2 shell has 4 orbitals: 1s and 3p orbitals.

The total number of orbitals in the n=3 level is given by n^2 = 3^2 = 9.

The total number of orbitals in a shell is given by n^2. For n=4, it is 4^2 = 16.

Four quantum numbers (n, l, m_l, s) are required to completely describe an electron in an atom.

Atomic radius increases down a group due to the addition of electron shells.

The atomic radius increases as you move down the group of alkali metals.

Electronegativity increases from left to right across a period.

Ionization energy decreases as you move down the group in s-block elements due to increased atomic size.

Ionization energy decreases down the group for alkali metals.

Metallic character decreases from left to right across a period.

S-block metals typically form ions with a charge of +2.

The unit of electric charge is the Coulomb.