CHM 101 – General Inorganic Chemistry

This set of flashcards covers the key concepts of matter, states of matter, properties, the mole concept, atomic masses, gas laws, and types of chemical reactions as discussed in the General Inorganic Chemistry course.

What is matter?

Matter is any substance which has mass and occupies space.

What are the four states of matter?

Solid, liquid, gas, and plasma.

What defines a solid?

Solids have a definite shape and volume, with particles held closely together.

How do liquids differ from solids?

Liquids have a definite volume but no definite shape, allowing particles to move more freely.

Describe gases in terms of their properties.

Gases have neither fixed shape nor volume; particles move freely and are far apart.

What is plasma?

Plasma is a superheated gas with no definite volume or shape, consisting of free-moving ions and electrons.

What are physical properties of matter?

Characteristics like color, hardness, malleability, and boiling/melting points that do not change the identity of the substance.

What are chemical properties of matter?

Characteristics that involve a change in the identity of the substance, such as flammability and reactivity.

What is a pure substance?

A substance with a constant composition made of one kind of particle.

Differentiate between elements and compounds.

An element cannot be broken down into simpler substances, while a compound consists of two or more elements chemically combined.

What is a mixture?

A combination of two or more substances that can be separated by physical methods.

What distinguishes homogeneous mixtures from heterogeneous mixtures?

Homogeneous mixtures have uniform composition throughout, while heterogeneous mixtures have varying properties in different areas.

What defines an ion?

An ion is an atom or group of atoms that has a net electric charge.

What are cations and anions?

Cations are positively charged ions; anions are negatively charged ions.

What is the mole concept?

The mole is a measure that contains 6.022 x 10^23 particles, corresponding to the number of atoms in 12 grams of carbon-12.

Define relative atomic mass.

The average mass of an atom of an element compared to 1/12 of the mass of a carbon-12 atom.

What does the ideal gas law describe?

The relationship among pressure, volume, temperature, and number of moles of an ideal gas.

What is Dalton's law of partial pressures?

The total pressure in a mixture of non-reacting gases equals the sum of their individual partial pressures.

Explain Boyle's Law.

At constant temperature, the volume of a gas is inversely proportional to its pressure.

What distinguishes chemical equations?

Chemical equations are symbolic representations of chemical reactions showing reactants and products with their states.

What characterizes a combination reaction?

A reaction where two or more reactants combine to form a single product.

What example illustrates a decomposition reaction?

A single reactant breaks down into two or more products, like magnesium hydroxide decomposing into magnesium oxide and water.

Define stoichiometry.

Stoichiometry involves calculations based on balanced chemical equations to relate quantities of reactants and products.