Second semester review
Classification
Heterotrophic/ Autotrophic (TEKS 6.12D)*

Heterotrophic/ Autotrophic
o Heterotrophic- gets nutrition from an outside source
 Examples are anything that eats: consumers, animals, bacteria, fungi
o Autotrophic- self feeder; makes own food through photosynthesis or chemosynthesis
 Examples are producers; plants and some acheabacteria
Domains, Kingdoms (TEKS 6.12C)

Levels of Organization (Domains, Kingdoms)
ARCHEA
BACTERIA
Archeabacteria
Eubacteria
Three DOMAINS that contain kingdoms
EUKARYA
Plants, animals,
fungi, protist
Unicellular/Multi-cellular (TEKS 6.12D)*

Organisms are composed of one or more cells: Unicellular/ Multi-cellular
o Unicellular- one celled organisms; the individual organism is made up of only one
cell like bacteria.
o Multi-cellular- many celled organisms; the organism is made up of many cells
working together like humans.
 Cellstissuesorganssystemsorganism
Mode of Reproduction (TEKS 6.12D)*
o Sexual reproduction
 Sex cells are created through meiosis
 makes 4 daughter cells with half the genetic information
 Needs the genetic information of two parents to create a unique
organism allowing for more genetic variation.
o Asexual reproduction



Requires the genetic of only one parent
Offspring is genetically identical to the parent
Types of asexual reproduction:
 Budding – organism grows out of the adult
 Binary fission- like mitosis, occurs in bacteria
 Parthenogenesis- whip tail lizards in New Mexico are all females and
lay eggs that hatch to be clones of the mother.
 Regeneration- The regrowth of a missing limb, like lizard tails and
starfish.
Chemistry
Atoms (TEKS 6.5A)

Atoms
o Basic building block of all matter
o Smallest part of an element that still holds the properties of that element.
Elements comprise Earth (TEKS 6.5B)
Elements, Compounds (TEKS 6.5C)*
o Elements- A substance consisting of atoms which all have the same number of protons i.e. the same atomic number. Elements are chemically the simplest form.
 Examples- H, O, C, He, Cl, Na,
o Compound- a substance formed by the chemical combination of two or more elements in
fixed proportions.
 Examples- H2O, C6H12O6
Review Physical Properties (TEKS 5.5A)
o
Properties that can be measured or seen through direct observation, include;
 Size
 Texture

 Color
 State (S,L,G)

 Luster
 Malleability

 Density
 Magnetism

 Mass
 Specific
 Volume
gravity
 Length
 Conductivity
Temperature
Hardness
Cleavage
Fracture
Physical vs. Chemical Properties/Changes (TEKS 6.5D)
Phase Change – aka change in state of matter – a PHYSICAL CHANGE
1.
2.
3.
4.
Melting point – solid state to liquid state (heat is added)
Boiling point – liquid state to gas state (heat is added)
Freezing point – liquid state to solid state (heat is removed)
Condensation point – gas state to liquid state (heat is removed)
o Physical change- A physical change involves a change in physical
properties.
 Examples of physical properties include:
 Melting
 textural change
 transition to a gas
 Shape
 change of strength
 Size
 change of
 Color
durability
 Volume
 changes to crystal
 Density
form
o
Chemical properties - Properties that can only be observed when one
substance changes into a different substance.
o
Chemical changes- alter the composition of the original matter. Different
elements or compounds are present at the end of the chemical
change. The atoms in compounds are rearranged to make new and
different compounds.
 Examples of a chemical change:


Example- If you leave an iron nail outside, it will eventually rust.
A chemical property of iron is that it reacts with oxygen (O2) in the
air to form rust, also known as iron oxide (Fe2O3).


Burning paper
Photosynthesis


Cooking
Lighting a match

Indications that a chemical change may have occurred are:
 Change is difficult or impossible to reverse
 Change in temperature
 Precipitate (solid) formation in a liquid
 Bubbles
 Emission of light
 Emission of sound
Density Calculations (TEKS 6.6B)*
Density = mass divided by volume (D=m/V)
o Formula:
 Density = mass/volume
 If an object has a mass of 4g and volume of 2 ml, then its density will be
expressed as
 d = m/v
 d = 4g/2ml
 d = 2 g/ml
Metal/ Non-metal/ Metalloids (TEKS 6.6A)*
Type
Metal
Metalloid
Luster
Yes
Slight luster
Malleability
Yes
brittle
Nonmetal
dull
brittle
Conductivity
Yes
only conducts electricity
in special circumstances
nonconductive
o Metals-

 Shiny (luster),
 Most are solid at room temperature,
 Ductile – can be made into wire.
 Malleable- can be shaped with a hammer without shattering
 Good conductors of heat and electricity
Examples:
 Al
 Fe
 Ag
 Cu
 Au
o Nonmetals Most are gases
 Some are brittle solids
 Poor conductors of heat and electricity
 Examples:
 S
 Fl
 O
o Metalloids Metalloids are elements that:
 Have properties between those of metals and nonmetals.
 Semiconductors


For example, the element silicon (Si), a metalloid. Silicon, a solid at
room temperature, can conduct heat and electricity, although not as
easily as many metals. However, silicon is very brittle (not malleable).
Silicon easily chips and shatters in its pure form. And like metals Silicon
has luster (shiny). It is used in electronics, as in computer chips. Also,
silicon dioxide (a compound of silicon) is used to make glass.
Examples:
 Si
 As
 Te
Periodic Table
o
o
o
o
Provides a way to organize all the known elements.
Organizes the elements according to how they combine with other elements (chemical
properties).
Is organized in order of increasing atomic number instead of atomic weight.
Divided into periods and groups.
 Periods –
 Each horizontal row is called a period
 Groups –
 Each vertical column is called a group or family. Groups of
elements have similar properties.
Symbols (TEKS 6.5A)
o
The chemical symbol of an element is a one-, two-, or three-letter symbol that
represents an element in the periodic table and in chemical formulas.
 Examples:
 H- hydrogen
 Fe- Iron
Only elements are on found on the Periodic Table (TEKS 6.5C)*
Location of metal/nonmetal/metalloid (TEKS6.6A)*
Non-metals
Metals
Energy
Energy types
Potential/stored/positional
 Biomass (chemical potential)
 Gravitational (positional)
 Nuclear
Kinetic/mechanical
 Geothermal
 Thermal aka heat
 Radiant aka light/solar (any wave/ray from
electromagnetic spectrum)
 Electrical energy
 Wind
 Sound
 Hydropower including Tidal power
Energy Resources
Nonrenewable
Fossil Fuels
 Oil/petroleum
 Coal
 Natural gas
Nuclear fuel
 Uranium
 Plutonium
Renewable
Air
(wind)(mechanical)
Alternative
Wind
Biofuel aka biomass
Plants/animals (biofuels)(chemical)
Water (hydropower)(potential)
Hydroelectric
Radiant aka solar
Geothermal (magma)
Forces and Motion
Balanced forces = net force of zero = no motion
Unbalanced forces cause all motion

Identify and describe the changes in position, direction, and speed of an object when
acted upon by unbalanced forces
o

Calculate average speed using distance and time measurements
o For example;

Find the speed if:

Distance = 360 m and the time = 1 h remember
60 minutes)
S= d/t
S= 360 m/60 s
S= 6 m/s
(1 hour =

Compare and contrast potential and kinetic energy
o Total Energy = Potential Energy + Kinetic Energy

Investigate how inclined planes and pulleys can be used to change the amount of
force to move an object
o Inclined plane-

o Pulley systems