States of Matter and Properties Quiz

States of Matter

• Solids have a fixed volume and shape. Particles are tightly packed in a regular array.
• Liquids have a fixed volume but take the shape of their container. Particles are close together but can move around.
• Gases have no fixed volume or shape; they expand to fill their container. Particles are far apart and move randomly.

Physical and Chemical Properties/Changes

• Physical properties can be observed without changing the substance's composition. Examples include boiling point, melting point, color, and odor.
• Physical changes alter the appearance or state of a substance without changing its chemical composition. Examples include melting ice, boiling water, and dissolving sugar in water.
• Chemical properties describe how a substance reacts with other substances or how it changes into other substances.
• Chemical changes (reactions) involve the transformation of one or more substances into new substances.
• Examples include burning paper, metabolizing food, and combining oxygen and hydrogen to form water.

Pure Substances and Mixtures

• Pure substances are composed of only one kind of particle (element or compound).
• A pure substance has a constant composition.
• Examples of pure substances include water (H₂O) and table sugar (C₁₂H₂₂O₁₁).
• Mixtures are composed of more than one substance.
• Their composition varies, and they can be physically separated.
• Examples include a salad, saltwater, and air.

Elements and Compounds

• Elements are pure substances that cannot be broken down into simpler substances by chemical means.
• Compounds are pure substances formed by chemically combining two or more different elements.

Matter

• Matter is anything that has mass and takes up space.

Chemistry

• Chemistry is the study of matter, its composition, properties, and transformations.

Significant Figures

• Significant figures are the digits in a measured value that are known with certainty plus one estimated digit.
• Rules for determining significant figures include nonzero digits are always significant, zeros between nonzero digits are significant, zeros at the end of a number to the right of the decimal point are significant, but zeros at the end of a number without a decimal point are usually not significant.

Scientific Notation

• A way of expressing very large or very small numbers in a concise form as a product of a number between 1 and 10 and a power of 10.

Density

• Density is the mass of a substance per unit volume.
• Density is calculated by dividing the mass of a substance by its volume.

Volume Displacement

• The volume of an object can be determined by measuring the volume of water displaced when the object is submerged.

Specific Gravity

• Ratio of the density of a substance to the density of water.

Conversion Factors

• Used to convert a measurement from one unit to another.

Percentages

• A way of expressing a part of a whole. (%= part/whole)*100

Temperature Conversions

• Methods to convert between different temperature scales (Celsius, Fahrenheit, Kelvin).

Atoms and Subatomic Particles

• Atoms are made up of protons, neutrons, and electrons.
• Protons are positively charged, neutrons are neutral, and electrons are negatively charged.
• Protons and neutrons are located in the nucleus of an atom, and electrons orbit around the nucleus.
• The atomic number of an element represents the number of protons, while the mass number represents the total number of protons and neutrons.

Atomic Mass Number

• The sum of the number of protons and neutrons in an atom's nucleus.