science exam

What are the main branches of science mentioned in Chapter 1?

• Chemistry
• Astronomy
• Geology
• Biology

What are the steps of the Scientific Method?

1. Observe
2. Hypothesis
3. Experiment
4. Conclusion
5. Theory

Independent vs. Dependent Variables

• Independent Variable: The variable that is intentionally changed in an experiment to observe its effect.
• Dependent Variable: The variable that is being tested and measured; it changes in response to the independent variable.

Scientific Notation Example

Used to express very large or very small numbers, such as 1.23 \times 10^{23} or 3.4 \times 10^{12}.

SI Units and Temperature Conversions

Physical Science involves measuring in units like meters and grams, and converting between temperature scales: Celsius, Fahrenheit, and Kelvin.

Substance vs. Mixture

• Substance: Matter that has a uniform and definite composition (Elements and Compounds).
• Mixture: A physical blend of two or more components that can be separated by physical means.

Homogeneous vs. Heterogeneous Mixtures

• Homogeneous: A mixture that is uniform in composition; components are evenly distributed (e.g., solution).
• Heterogeneous: A mixture that is not uniform; components are visibly different (e.g., suspension).

Element vs. Compound

• Element: The simplest form of matter that has a unique set of properties (e.g., Oxygen).
• Compound: A substance that contains two or more elements chemically combined in a fixed proportion (e.g., H_{2}O).

Solution, Suspension, and Colloid

• Solution: A homogeneous mixture with very small particles that do not settle.
• Suspension: A heterogeneous mixture with large particles that settle over time.
• Colloid: A mixture with intermediate-sized particles that do not settle and scatter light.

Physical vs. Chemical Properties and Changes

• Physical: Properties observed without changing the substance's identity (melting point, density); changes only affect appearance (melting, boiling).
• Chemical: The ability of a substance to undergo a specific chemical change (flammability, reactivity); changes result in new substances (burning, rusting).

Density and Volume Equations

• Density (D): D = M / V
• Volume (V): V = M / D or V = l \times w \times h

Filtration vs. Distillation

• Filtration: Separates a solid from a liquid in a heterogeneous mixture.
• Distillation: Separates components of a homogeneous mixture based on their different boiling points.

What are the five states of matter?

1. Solids
2. Liquids
3. Gases
4. Plasma
5. BEC (Bose-Einstein Condensate)

Kinetic Theory of Matter

All matter consists of tiny particles that are in constant, random motion; the speed of particles determines the state of matter.

Boyle’s, Charles’s, and Gay-Lussac’s Gas Laws

• Boyle’s Law: Pressure and Volume (P{1}V{1} = P{2}V{2}).
• Charles’s Law: Volume and Temperature (\frac{V{1}}{T{1}} = \frac{V{2}}{T{2}}).
• Gay-Lussac’s Law: Pressure and Temperature (\frac{P{1}}{T{1}} = \frac{P{2}}{T{2}}).

Phase Changes

• Sublimation: Solid to Gas
• Condensation: Gas to Liquid
• Vaporization: Liquid to Gas
• Melting: Solid to Liquid
• Boiling: Occurs when vapor pressure equals atmospheric pressure.

What are the main branches of science mentioned in Chapter 1?

• Chemistry
• Astronomy
• Geology
• Biology

What are the steps of the Scientific Method?

1. Observe
2. Hypothesis
3. Experiment
4. Conclusion
5. Theory

Independent vs. Dependent Variables

• Independent Variable: The variable that is intentionally changed in an experiment to observe its effect.
• Dependent Variable: The variable that is being tested and measured; it changes in response to the independent variable.

Scientific Notation Example

Used to express very large or very small numbers, such as 1.23 \times 10^{23} or 3.4 \times 10^{12}.

SI Units and Temperature Conversions

Physical Science involves measuring in units like meters and grams, and converting between temperature scales: Celsius, Fahrenheit, and Kelvin.

Substance vs. Mixture

• Substance: Matter that has a uniform and definite composition (Elements and Compounds).
• Mixture: A physical blend of two or more components that can be separated by physical means.

Homogeneous vs. Heterogeneous Mixtures

• Homogeneous: A mixture that is uniform in composition; components are evenly distributed (e.g., solution).
• Heterogeneous: A mixture that is not uniform; components are visibly different (e.g., suspension).

Element vs. Compound

• Element: The simplest form of matter that has a unique set of properties (e.g., Oxygen).
• Compound: A substance that contains two or more elements chemically combined in a fixed proportion (e.g., H_{2}O).

Solution, Suspension, and Colloid

• Solution: A homogeneous mixture with very small particles that do not settle.
• Suspension: A heterogeneous mixture with large particles that settle over time.
• Colloid: A mixture with intermediate-sized particles that do not settle and scatter light.

Physical vs. Chemical Properties and Changes

• Physical: Properties observed without changing the substance's identity (melting point, density); changes only affect appearance (melting, boiling).
• Chemical: The ability of a substance to undergo a specific chemical change (flammability, reactivity); changes result in new substances (burning, rusting).

Density and Volume Equations

• Density (D): D = M / V
• Volume (V): V = M / D or V = l \times w \times h

Filtration vs. Distillation

• Filtration: Separates a solid from a liquid in a heterogeneous mixture.
• Distillation: Separates components of a homogeneous mixture based on their different boiling points.

What are the five states of matter?

1. Solids
2. Liquids
3. Gases
4. Plasma
5. BEC (Bose-Einstein Condensate)

Kinetic Theory of Matter

All matter consists of tiny particles that are in constant, random motion; the speed of particles determines the state of matter.

Boyle’s, Charles’s, and Gay-Lussac’s Gas Laws

• Boyle’s Law: Pressure and Volume (P{1}V{1} = P{2}V{2}).
• Charles’s Law: Volume and Temperature (\frac{V{1}}{T{1}} = \frac{V{2}}{T{2}}).
• Gay-Lussac’s Law: Pressure and Temperature (\frac{P{1}}{T{1}} = \frac{P{2}}{T{2}}).

Phase Changes

• Sublimation: Solid to Gas
• Condensation: Gas to Liquid
• Vaporization: Liquid to Gas
• Melting: Solid to