Term 1 Exam Review (Honors Physical Science)

What is physical science?

A combination of physics and chemistry

scientifc theory

a possible explanation for repeatedly observed patterns in nature supported by observations and results from many investigations

scientific law

A statement that describes what scientists expect to happen every time under a particular set of conditions

Precision

a measure of how close a series of measurements are to one another

Accuracy

how close a measurement is to the true value

area

The number of square units required to cover a surface.

Volume

The amount of space an object takes up

Mass

the amount of matter in an object

Scientific Method Steps

Question, Research, Hypothesis, Experiment, Analyze the Data, Conclusion

independent variable

variable that is manipulated

dependent variable

The measurable effect, outcome, or response in which the research is interested.

control group

In an experiment, the group that is not exposed to the treatment; contrasts with the experimental group and serves as a comparison for evaluating the effect of the treatment.

qualitative data

descriptive data

quantitative data

numerical data

What is an SI unit?

International System of Units

What are the metric units?

Kilo, Hecto, Deca, Base, Deci, Centi, Milli, Micro (Kings Hate Dragons Because Dragons Can't Make Money).

Dimensional analysis

a technique of problem-solving that uses the units that are part of a measurement to help solve the problem

DRY MIX

Dependent

Responding

Y Axis

Manipulated

Independent

X Axis

scientific notation

A mathematical method of writing numbers using powers of ten.

significant figures

All the digits that can be known precisely in a measurement, plus a last estimated digit

matter

Anything that has mass and takes up space

Element

A pure substance made of only one kind of atom

Atom

Smallest particle of an element

Compound

A substance made up of atoms of two or more different elements joined by chemical bonds

molecule

smallest unit of most compounds

chemical formula

A combination of chemical symbols and numbers to represent a substance

pure substances

elements and compounds

Mixtures

A combination of two or more substances that are not chemically combined

melting point

the temperature at which a solid changes to a liquid

boiling point

The temperature at which a liquid boils

Density

mass/volume

Reactivity

How readily a substance combines chemically with other substances.

Flammability

the ability to burn

heterogeneous mixture

A mixture in which different materials can be distinguished easily

homogeneous mixture

A mixture in which substances are evenly distributed throughout the mixture

Miscible

Describes two liquids that are soluble in each other

Immiscible

liquids that are not soluble in each other

extensive property

a property that depends on the amount of matter in a sample

intensive property

a property that depends on the type of matter in a sample, not the amount of matter

chemical propety

a characteristic that describes how a substance changes into a different substance

physical change

A change in a substance that does not change its identity

chemical change

A change in matter that produces one or more new substances

Kinetic Molecular Theory

based on the idea that particles of matter are always in motion

temperature

A measure of how hot or cold something is.

thermal energy

Heat energy

Evaporation

Liquid to gas

Sublimation

solid to gas

Condensation

Gas to liquid

Freezing

liquid to solid

Endothermic

Absorbs heat

Exothermic

Releases heat

How can matter be classified?

elements, compounds, mixtures

Celsius to Kelvin

K=C+273

mass volume and density triangle

Mole Calculations formula

Number of moles = given mass / gram-formula (molar) mass

Democritus

Original idea of the atom

Dalton's Atomic Theory

1) elements are composed of atoms. 2) atoms of same element are identical, but differ from other elements. 3) elements can mix together 4) atoms only change when mixed with other elements

Rutherford

Gold foil experiment, discovered nucleus

Thomson

discovered the electron

Proton

positively charged particle

Neutron

no charge

Electron

negatively charged particle

Isotopes

Atoms of the same element that have different numbers of neutrons

Ions

positively and negatively charged atoms

charge

protons-electrons

Mass of an atom

protons + neutrons

atomic number

the number of protons in the nucleus of an atom

atomic mass

Number of protons and neutrons

average atomic mass

the weighted average of the atomic masses of the naturally occurring isotopes of an element

average atomic mass formula

(Percent to decimal)(mass) + (percent to decimal)(mass)

1 mole=

6.02x10^23