Semester 1 Exam Notes

Page 1

Matter and Energy

The size of atoms

and molecules as well as the temperature of the substance determines the speed

of its particles.

Temperature

measures the average kinetic energy.

All matter is

made of atoms and molecules that are always in motion.

The laws of

conservation state that energy and matter cannot be created nor destroyed.

When ice melts to

form water, energy is absorbed.

Liquid particles

slide past each other, but are still packed together.

Plasma particles

have been broken down and are ionized.

Solid particles

are in a rigid, fixed structure.

Gas particles are

in constant motion and rarely stick together.

Chapter 3

Electron –

negatively charged subatomic particles

Nucleus – atom’s

central region

Proton –

positively charged subatomic particle

Neutron –

subatomic particle with no charge

Atomic number –

number of protons in a nucleus

Mass number – sum

of protons and neutrons in the nucleus

Isotope - differs in number of neutrons

Unified atomic

mass unit - ½ the mass C12

Orbital - region where electron are found

Valence electron – electron found in outermost shell

Photon – particle of light with no mass

Period – horizontal row of elements

Group – vertical column of elements

Ion – has gained or lost one or more electrons

Metal – shiny, conducts heat and electricity well

Nonmetal – conducts heat and electricity poorly

Semiconductor – conducts heat and electricity better

than an insulator, but not as good as a

conductor

Noble gases – Helium, Argon, Krypton, Xenon, Radon

Chapter 2

Inference

– a conclusion based upon evidence or reasoning

Flammability

– the ability to burn

Chemical

property - describes how a substance

changes into a new one with different properties

State

– Solid, liquid, gas, plasma are all examples of this

Reactivity

– The ability to chemically combine with another substance

Density

– Mass/Volume or g/cm3

Immiscible

– a liquid that cannot be mixed

Miscible

- liquid that is able to be mixed

Homogenous

mixture – components of a mixture are evenly distributed

Heterogeneous mixture – components of

a mixture are unevenly distributed

Subscript – Such as the 2

in H2O

Compound – made up of two or more

different elements joined by elemental bonds

Molecule – a group of atoms held

together by chemical forces; smallest unit of matter that can exist by itself

and retain all of a substance’s chemical properties

Atom – the smallest unit of an

element that maintains the chemical properties of that element

Element – Hydrogen, oxygen, neon,

etc. are all examples of this

Matter – has mass; takes up space

Elements

Sodium – Na

Iron – Fe

Copper – Cu

Silver- Ag

Tin – Sn

Tungsten – W

Gold – Au

Mercury – Hg

Lead – Pb

SI Unit Prefixes

Prefix

Symbol

Meaning

Kilo-

K

1,000

Mega-

M

1,000,000

Giga-

G

1,000,000,000

Deci-

d

0.1

Centi-

c

0.01

Milli-

m

0.001

Micro-

μ

0.000001

Nano-

n

0.000000001

Chapter 2 Vocabulary

Inference

– a conclusion based upon evidence or reasoning

Flammability

– the ability to burn

Chemical

property - describes how a substance

changes into a new one with different properties

State

– Solid, liquid, gas, plasma are all examples of this

Reactivity

– The ability to chemically combine with another substance

Density

– Mass/Volume or g/cm3

Immiscible

– a liquid that cannot be mixed

Miscible

- liquid that is able to be mixed

Homogenous

mixture – components of a mixture are evenly distributed

Heterogeneous mixture – components of

a mixture are unevenly distributed

Subscript – Such as the 2

in H2O

Compound – made up of two or more

different elements joined by elemental bonds

Molecule – a group of atoms held

together by chemical forces; smallest unit of matter that can exist by itself

and retain all of a substance’s chemical properties

Atom – the smallest unit of an

element that maintains the chemical properties of that element

Element – Hydrogen, oxygen, neon,

etc. are all examples of this

Matter – has mass; takes up space

Physical Science Semester 1 Exam

Notes

States of Matter

Solids have a

definite shape and volume.

Five changes of

state:

Evaporation –

Liquid to gas

Condensation –

gas to liquid

Melting – solid

to liquid

Freezing – liquid

to solid

Sublimation –

solid to gas

Viscosity – a liquid’s

resistance to flow; caused by particle attraction

Wood floats on

water because it is less dense than water

Three gas laws:

Boyle’s Law –

fixed temperature; volume and pressure have a inversely proportional relationship

Charles’ Law –

fixed pressure; volume and temperature have a direct relationship

Gay-Lussac’s Law –

fixed volume; temperature and pressure have a direct relationship

Notes

Vocabulary