Term
| Name the 3 states of matter |
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Definition
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Term
| Give characteristics of a Solid. |
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Definition
- Fixed shape and vol. Most dense, incompressible
- Particles are unable to move from one spot to another OR cnt undergo translational motion.
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Term
| Give characteristics of a Liquid. |
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Definition
- Fixed vol.
- flows to conform shape of a container.
- middle density
- relatively compressible
- Particles have ability to move from one place to another.
- Close to eachother but not as close as a solid.
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Term
| Give characteristics of Gas. |
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Definition
- No fixed shape.
- expands to fill container
- lowest density
- compressible
- Particles are very far apart moving freely
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Term
| Name transitions between the state of matter. |
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Definition
- Solid to Liquid: melting
- Liquid to Gas: evaporation
- Solid to Gas: sublimation
- Liquid to Solid: freezing or solidify
- Gas to Liquid: condensation
- Gas to Solid: deposition
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Term
| List the three phases of matter in order from low density to high density |
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Definition
Solid typically denser than liquid which is denser than gas |
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Term
| Name and explain two differences between a "pure substance" and a "mixture" |
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Definition
Pure Substance Mixture
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-one component -More than 1 component
-fixed composition -variable composition
-definite properties -can seperate via physical means
-cant be separated via -properties depend on composition
physical mean -components retain own properties |
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Term
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Definition
Made of two or more different kinds of atoms bonded together in a fixed whole number ratio |
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Term
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Definition
| consists of only one type of atom |
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Term
| Explain homogeneous mixture. |
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Definition
| has the same composition throughout |
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Term
| Explain heterogeneous mixture. |
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Definition
| has different compositions depending upon sampling site |
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Term
| How can you tell the difference between a physical and chemical change? |
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Definition
A physical change involves the physical state or phase. A physical change can usually be
reversed easily and no new substances are produced. Examples: dissolving, melting,
evaporating. On the other hand, a chemical change involves the creation of one or more new
substances with different properties. |
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Term
Chemical or Physical Property?:
Gold is shiny and yellowish in color |
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Definition
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Term
Chemical or Physical Property?:
Iron in steel rusts |
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Definition
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Term
Chemical or Physical Property?:
Table salt is soluble (dissolves) in water |
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Definition
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Term
Chemical or Physical Property?:
Sodium metal sparks when placed in water |
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Definition
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Term
| Subatomic particles – name them and tell their location in the atom. |
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Definition
Proton: in nucleus, positive, mass ~ 1 amu
Neutron: in nucleus, neutral, mass ~1 amu
Electron: outside nucleus, negative, mass ~ 0.0002 amu |
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Term
| What was Rutherford’s Experiment? What did the findings mean about the model of the atom |
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Definition
Small particles were shot at a thin piece of
gold foil. Some of the particles were deflected but most went straight through. He concluded that an
atom is mostly empty space with a small dense nucleus. The nucleus is positively charged and
contains most of the mass of the atom but occupies essentially none of the volume of the atom. |
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Term
| What were the main ideas of Dalton’s Theory? |
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Definition
- There are five main ideas to Dalton’s Atomic Theory
Elements are made of indivisible particles called atoms. (Not exactly, atoms themselves are composed of sub-atomic particles.)
All atoms of a given element are identical. (Not exactly, all atoms of a given element to first approximation have the same properties, but might have different masses due to a different number of
neutrons [isotopes].)
Atoms of a given element are different than those of any other element in both their properties
and in their masses.
Atoms of one element combine with atoms of other elements to form chemical compounds in
definite whole number ratios.
Atoms cannot be created, divided into smaller particles, nor destroyed in a chemical process.
The chemical reaction simply changes the way the atoms are grouped together. |
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Term
What Laws were used to come up with Dalton's atomic
theory? |
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Definition
- Dalton used the Law of Conservation of Mass and the Law of Constant Composition which is also
known as the Law of Definite Proportions |
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Term
| What is the difference between a Theory and a Law? |
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Definition
Theory is an explanation of the WHY or underlying reasons behind obsevations, experimental results, or laws.
A Law is a generalized statement that summarizes a set of related observations or experimental results. Both can be used for predicting future behavior. |
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Term
Explain how the following experiment does not violate the Law of Conservation of Mass:
Sealed jar with a piece of metal inside has a total mass of 125.675 g. After a period of time, the jar was
opened, then reclosed, and massed again.
Total mass after the experiment
was found to be
126.230 g. |
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Definition
As long as the jar was sealed the mass remains 125.675 g. Some gas in the sealed jar reacted with the
metal and increased the mass of the metal, but the total mass would be the same. (The jar remained
sealed.) As the jar was opened, NEW air enters the jar to replace the gas used in the reaction. (Think
of when you open something vacuum packed like coffee.) The mass, inside the jar, is therefore the
mass of the metal + the mass of reacted gas + the mass of NEW gas |
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