The electron configuration is determined solely by the element's mass number.

The electron configuration of an element is determined by its atomic number and follows the order of filling orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule.

The electron configuration can be found by looking at the periodic table without any calculations.

Electron configurations are random and do not follow any specific rules.

Ionic bonds involve electron transfer and attraction between ions, while covalent bonds involve electron sharing between atoms.

Ionic bonds occur only in metals, while covalent bonds occur only in non-metals.

Ionic bonds are formed by sharing electrons, while covalent bonds involve electron transfer.

Covalent bonds are stronger than ionic bonds due to their nature of attraction between ions.

sublimation, evaporation, condensation

neutralization, ionization, crystallization

synthesis, decomposition, single replacement, double replacement, combustion, redox

oxidation, hydrolysis, polymerization

Transparency

Brittleness

Low melting point

Common properties of metals include conductivity, malleability, ductility, luster, and high density.

Acids have a pH less than 7, and bases have a pH greater than 7.

Both acids and bases have a pH of 7.

Acids and bases have the same pH level.

Acids have a pH greater than 7, and bases have a pH less than 7.

Group 3

Group 18

Group 14

Group 1

Valence electrons are irrelevant in chemical reactions.

Valence electrons are significant in bonding because they determine how atoms interact and bond with each other.

Valence electrons only affect the mass of an atom.

Valence electrons are only important in ionic compounds.

Changes in mass or volume only

Presence of a solid in a liquid

No observable changes in the substance

Look for changes in color, temperature, gas production, precipitate formation, or odor change.

High reactivity with water

High density compared to transition metals

Non-reactive with air

Low melting point

Covalent bond

Hydrogen bond

Ionic bond

Metallic bond

The pH of the solution decreases.

The pH of the solution remains the same.

The pH of the solution fluctuates randomly.

The pH of the solution increases.

Alkali metals

Halogens

Noble gases

Transition metals

A catalyst changes the products of a chemical reaction.

A catalyst slows down a chemical reaction by increasing the activation energy.

A catalyst is a substance that is consumed in the reaction.

A catalyst speeds up a chemical reaction by lowering the activation energy.

A reaction is exothermic if it produces light and endothermic if it produces sound.

Exothermic reactions always occur at low temperatures, while endothermic reactions occur at high temperatures.

A reaction is exothermic if it releases heat and endothermic if it absorbs heat.

A reaction is exothermic if it absorbs heat and endothermic if it releases heat.

Weak acids have a higher pH than strong acids.

Strong acids completely dissociate in solution, while weak acids only partially dissociate.

Weak acids do not conduct electricity, while strong acids do.

Strong acids are always corrosive, while weak acids are not.

Increasing temperature decreases the reaction rate.

Increasing temperature generally increases the reaction rate.

Temperature has no effect on the reaction rate.

Decreasing temperature always increases the reaction rate.

The periodic table organizes elements based on their atomic mass only.

The periodic table provides information about the properties and relationships of elements.

The periodic table is used solely for predicting chemical reactions.

The periodic table lists only metals and ignores non-metals.

Electrons are tightly bound to individual atoms.

Electrons are delocalized and free to move throughout the structure.

Electrons are transferred from one atom to another.

Electrons are shared between atoms.

Calcium

Oxygen

Chlorine

Argon

Increasing concentration only affects solid reactants.

Increasing concentration generally increases the reaction rate.

Increasing concentration has no effect on the reaction rate.

Increasing concentration generally decreases the reaction rate.

Electrons are transferred between atoms.

Electrons are localized around a single atom.

Electrons are shared between atoms.

Electrons are completely free and not associated with any atom.

The pH of the solution fluctuates randomly.

The pH of the solution decreases.

The pH of the solution remains the same.

The pH of the solution increases.

Decomposition reaction

Synthesis reaction

Single replacement reaction

Double replacement reaction

Noble gases are highly reactive and readily form compounds.

Noble gases have a full valence shell, making them mostly inert.

Noble gases are all solid at room temperature.

Noble gases are found in Group 1 of the periodic table.