Questions and Answers
What is the process called when a solid transforms directly into a gas?
Which of the following is an example of deposition?
What are the three states of matter?
Solid, liquid, gas
What is a pure substance?
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Heterogeneous mixtures have only one phase.
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What describes intrinsic properties of matter?
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Who is associated with the Law of Conservation of Mass?
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The 4th state of matter is called _____
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What is the process of changing a solid directly to a gas called?
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Deposition is the process of changing gas directly to solid.
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What is the simplest form of substance known as?
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Which type of mixture consists of two or more substances wherein individual substance identities are retained?
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A _________ is made up of two or more chemicals united in a fixed ratio.
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Match the following terms with their definitions:
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What is the law that states mass or matter is always constant?
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Study Notes
Sublimation and Deposition
- Sublimation refers to the phase transition of matter from solid to gas (e.g., naphthalene balls).
- Deposition is the transition from gas to solid (e.g., dry ice).
Phases of Matter
- Matter is classified into solid, liquid, and gas based on properties.
- Solid: definite shape and volume, non-compressible.
- Liquid: indefinite shape, assumes the shape of the container, has a definite volume, non-compressible.
- Gas: indefinite shape and volume, highly compressible.
Matter Classification
-
Pure Substance:
- Divided into elements (simplest form) and compounds (two or more chemicals united, separable by chemical means).
-
Mixture:
- Comprises two or more substances where individual identities are retained, separable by physical means (e.g., distillation of alcohol and water).
- Classified into:
- Homogeneous (one phase; solution)
- Heterogeneous (two phases; suspension or colloid, e.g., milk)
Plasma
- Plasma is the fourth state of matter and the most abundant state in the universe.
- Contains free-moving ions and electrons, making it susceptible to magnetic fields.
- Examples include ionized neon light, auroras, stars, and the sun.
Properties of Matter
-
Extrinsic Properties:
- Dependent on the amount of matter present; examples include length, mass/weight, volume, pressure, entropy, enthalpy, and electrical resistance.
-
Intrinsic Properties:
- Independent of the amount of matter; examples include density (e.g., water = 1 g/mL), viscosity, velocity, temperature, and color.
Phase Changes
- Phase changes include transitions between solid, liquid, gas, and plasma states.
- The order of intermolecular forces affects the stability of these phases:
- Ionization strength: Solid > Liquid > Gas > Plasma
- Enthalpy (heat/reaction energy): Plasma > Gas > Liquid > Solid
Fundamental Chemistry Laws
-
Law of Conservation of Mass (Matter):
- Proposed by Antoine Lavoisier, stating that mass/matter remains constant; it cannot be created or destroyed in a chemical reaction.
Sublimation and Deposition
- Sublimation refers to the phase transition of matter from solid to gas (e.g., naphthalene balls).
- Deposition is the transition from gas to solid (e.g., dry ice).
Phases of Matter
- Matter is classified into solid, liquid, and gas based on properties.
- Solid: definite shape and volume, non-compressible.
- Liquid: indefinite shape, assumes the shape of the container, has a definite volume, non-compressible.
- Gas: indefinite shape and volume, highly compressible.
Matter Classification
-
Pure Substance:
- Divided into elements (simplest form) and compounds (two or more chemicals united, separable by chemical means).
-
Mixture:
- Comprises two or more substances where individual identities are retained, separable by physical means (e.g., distillation of alcohol and water).
- Classified into:
- Homogeneous (one phase; solution)
- Heterogeneous (two phases; suspension or colloid, e.g., milk)
Plasma
- Plasma is the fourth state of matter and the most abundant state in the universe.
- Contains free-moving ions and electrons, making it susceptible to magnetic fields.
- Examples include ionized neon light, auroras, stars, and the sun.
Properties of Matter
-
Extrinsic Properties:
- Dependent on the amount of matter present; examples include length, mass/weight, volume, pressure, entropy, enthalpy, and electrical resistance.
-
Intrinsic Properties:
- Independent of the amount of matter; examples include density (e.g., water = 1 g/mL), viscosity, velocity, temperature, and color.
Phase Changes
- Phase changes include transitions between solid, liquid, gas, and plasma states.
- The order of intermolecular forces affects the stability of these phases:
- Ionization strength: Solid > Liquid > Gas > Plasma
- Enthalpy (heat/reaction energy): Plasma > Gas > Liquid > Solid
Fundamental Chemistry Laws
-
Law of Conservation of Mass (Matter):
- Proposed by Antoine Lavoisier, stating that mass/matter remains constant; it cannot be created or destroyed in a chemical reaction.
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Description
Test your knowledge on sublimation and its applications in pharmaceutical chemistry. This quiz covers fundamental concepts related to matter and general chemistry, providing a comprehensive review for students. Ideal for those studying the PHLE curriculum.
