Chemistry and atomic structure review

Comprehensive vocabulary flashcards covering chemical bonding, acid-base properties, periodic trends, and reaction types based on the lecture notes.

1 part per billion ($ppb$)

A measurement approximately represented by adding a single drop of solute to a swimming pool.

pH of $0.034\,mol/L$ sodium hydroxide ($NaOH$)

$$12.5$$

Concentration of hydrochloric acid at pH $4.3$

$$5.0 \times 10^{-5}\,M$$

Water ($H_2O$) Geometry

A bent, polar molecule containing polar bonds and two pairs of lone electrons.

Solubility of ionic solutes

Occurs when ions in ionic compounds have a greater attraction to water than to their neighboring ions.

Molarity ($M$)

The concentration of a solution, calculated as moles of solute per liter of solvent; for example, $8.3\,mol$ copper (II) sulfate in $3.0\,L$ water is $2.8\,M$.

Partial pressure of nitrogen

Calculated as $95.94\,kPa$ when nitrogen is collected over water at $26.0^{\circ}C$ with a total pressure of $99.3\,kPa$.

Benzene

A nonpolar substance that is insoluble in water.

Hydrogen bonding

The intermolecular force responsible for water's unusually high boiling point.

Beakers

Glassware that is not accurate for precise volume measurements; graduated cylinders, pipettes, or burettes are preferred.

Burette

A device used to perform a titration to measure the volume of a liquid or gas.

Phenolphthalein

An indicator used in acid-base titrations that turns pink in basic solutions to detect the endpoint.

Chlorination

A method of water supply treatment that has a low retention rate in water and is used to eliminate water-borne diseases.

Conjugate acid-base pair

A pair of substances related by the gain or loss of a proton, such as ammonia ($NH_3$) and ammonium ($NH_4^+$).

Micelle particle

An important component of soap that can assist in cleaning by interacting with both polar and non-polar substances.

Covalent bond

A type of chemical bond formed by elements such as bromine ($Br$) and hydrogen ($H$), or carbon ($C$) and phosphorus ($P$).

Ionic bond

A chemical bond resulting from the attraction between oppositely charged ions, formed by elements such as magnesium ($Mg$) and oxygen ($O$).

Electrolytes

Substances that can conduct electricity in both molten form and in solution.

Cations

Atoms or molecules that have lost electrons to develop a positive ($+$) charge.

Nitrous acid

$$HNO_2(aq)$$

Hydrobromic acid

$$HBr(aq)$$

Copper(II) oxide

$$CuO$$

Lithium sulfate

$$Li_2SO_4(aq)$$

Hydrogen peroxide

$$H_2O_2(l)$$

Copper(II) nitrite

$$Cu(NO_2)_2(aq)$$

Sodium ($Na$)

A metal identified as being more reactive in water compared to aluminum, magnesium, or silver.

First Ionization Energy

The energy required to remove the first electron from an atom; Group 1 elements (like Element X) exhibit the lowest energy for this process.

Double displacement reaction

A reaction where two compounds exchange ions to form two new compounds, e.g., $Mg(OH)_2 + 2HNO_3 \rightarrow Mg(NO_3)_2 + 2H_2O$.

Single displacement reaction

A chemical reaction that must always occur in solution where one element replaces another in a compound.

Sulfate ion charge

$$-2$$

Electronegativity of fluorine

$$4.0$$

Hafnium

The element located in Group 4, Period 6 of the periodic table.

Alkali metals

The common name for Group 1 elements in the periodic table.

Atomic number

The number of protons found in the nucleus of an atom.

Isotopes

Atoms of the same element that have the same number of protons but a different number of neutrons.

Dissociation

The separation of ions that occurs as ionic compounds dissolve in water.

Nitric acid ($HNO_3$)

Classified as a strong acid because it possesses high electrical conductivity and ionizes more than $99\%$.

Acetic acid

A weak acid that ionizes less than $10\%$ in solution.

Weak base

A base that partially reacts with water to form hydroxide ions ($OH^-(aq)$).

Solute

The substance that is dissolved in a solvent; for example, sugar in a water solution or carbon dioxide in air.