7th Grade: Unit Notes!

CHEMISTRY—> MATTER

I. CLASSIFICATION OF MATTER

(These classification notes should be in a Graphic Organizer form, as we will be observing and classifying different types of substances and matter in class. YOU will come up with the examples of the Chemical and Physical Properties, as you observe the types of matter)

A. What are Physical Properties?

Definition: Physical properties are the characteristics that can be observed without changing the substance into another substance.

Ex.: Ripping or tearing, folding

B.  What are Chemical Properties?

Definition: Chemical properties are the characteristics that determine how it will react with other substances or change from one substance to another.  

1.  New substances are made!
2.  New Properties!

PHYSICAL                                                           CHEMICAL

texture                                                             reactivity

density                                                             explosive

Changes to state of matter-                         flammable

(NOT simply naming a state of matter!) oxidation

 viscosity                                                        corrosive

crystal shape                                               radioactive

conducts heat                                               tarnishes

amorphism                                                 baking changes

malleable             hardness                        toxicity

odor                     porous                            half-life

taste                      magnetic                       flash point

pH                         malleable                      accelerant ability (fire)                     

flexible                conducts electricity          chromatography

porous                  clarity photosynthesis

density                 dissolves in H2O-solubility

melting point        opacity       

boiling point          elasticity

freezing point        distillation point   

condensation point    

luster (glassy luster,

sparkling luster, metallic luster)     

ability to form mixtures (heterogeneous, homogeneous)

fractures (breaks unevenly)      

cleavage (breaks into even, flat shapes and plates)

ductility (ability to form into a wire)

compressibility

water-resistant

II. Measurement of Matter

III. States of Matter – Molecular Arrangement, Motion & Energy

(these notes are supposed to be “Sketch Notes,” as you were shown in class. Here are a couple of simple examples.)

2. What Happens to Molecules in Matter with a Change in Pressure?

Boyles’ Law – this is a “law” for gas molecules

Water Displacement – happens when pressure is put onto water (or a liquid)! The molecules are just moved out of the way of the impact or pressure:

2. What Happens to Molecules in Matter with a Change in Heat or Thermal Energy?

Charles’ Law

Heating Water – or another liquid produces bubbles of air, water vapor and then steam:

Science Notes: Boiling Water

What Happens to the Molecules in Ice When It is Heated? The bonds break and it becomes a liquid!

How Does an Ice Cube Melt? by Jessica Tu

IV. Types of Matter

{SketchNotes Style: YOU choose which drawings and sketches YOU will complete with these notes!}

A. Example of a teacher- created set of SketchNotes for Types of Matter:

B.  Pure Substances; Types of Matter

1. Made up of only one type of matter—
2. Has its’ own definite properties.
3. Every sample of that substance is the same

C. Atoms –  A smallest partical of an  element; a “building block” of the element

• a pure substance; a single type of matter
• made up of sub-atomic particles: protons, neutrons, electrons
• protons = p+ ; Electrons = – ; neutrons = (no charge)

D. Molecule = two or more atoms chemically joined together; pure substance

• 1 molecule may be 2 or more atoms of 1 element (ex: O₂ or O₃ )
• 1 molecule may be 2 or more atoms of different elements = 1 molecule of a compound

E. Element:  a pure substance that cannot be broken down into other substances

(see the Periodic Table of the Elements for examples)

•        1.  Properties of elements are very specific to each type of matter
• Periodic Table Real World Uses for each element
•       2.  Common elements all around us (you might draw or sketch a few of these)  

• O = oxygen      N= nitrogen     
• C = carbon       H = hydrogen
• Na = sodium       Au = gold

F.  Compound: a pure substance formed from chemical combinations of different elements

(you might draw or sketch a few of these)  

Examples-Compounds

• 1. Carbon Dioxide = CO₂
• 2. Water = H₂O
• 3. Ammonia = NH₃

G.  Mixtures: 2 or more substances that are physically joined (Stirring, shaking, …        

Substances keep their physical properties

1. Heterogeneous!   (commonly called “mixtures’ )

•         Individual parts of the mixture are visible
• Substances may be physically separated   

 2. Homogeneous Mixtures:   also called Solutions

•         The “best mixed” of all mixtures; appear so well blended, that they look like one substance
• The molecules in a homogeneous mixture are evenly distributed

H. The Periodic Table = Organized Elements

1. Interactive P Tables: 

• Elements PT in Groups
•  Photographic Periodic Table
• P Table Elements.wlonk
• Science Notes The Periodic Table

• 2. Organized by the relationships of the elements to one another
• 3. Families = columns; those elements have similar chemical and physical properties
  Ex.: Family 1 – highly reactive
  Ex.: Family 18 = Noble Gasses (do NOT React!)
• 4. Left to right on the table = larger atomic mass

5. Key: Element “box” on the Periodic Table

Notes – You Can Use for All Science Units!

Notes for the 7th Science 23-24 School Year

I. Claim Evidence Reasoning – CER With Reproductive, Behavioral and Physical Traits

II.  Types of Experiments!

A.  Control:

1. This experiment does not have any changes added.
2. This is the experiment that all others are compared to
3.  ex.:  think about the Flower Lab example we talked about in class.  The Control experiment was the flower placed only in water (no substances added).

B.  Independent Variable:

1.  The changed factor that you want to test
2.  The one change that is different from the control experiment.
3.  Change only one independent variable at a time.
4.  Equal amounts of the variable must be added
5. ex.:  think about the Flower Lab example we talked about in class.  The Independent Variable were the different substances added to the flower’s water.

C.  Dependent Variable:

1.  The measurable results
2.  These may change in each trial

III. Lab Safety –

this is a sample of a Graphic Organizer for your notes:

STEM ENGINEERING!

IV. STEM – Engineering Design Process.

{The notes below – are short summaries of each section of the EDP. Students in each class referred to the “STEM EDP Box Paper” Students noted details on their paper. The entire process is detailed and described on the

STEM EDP page on this Blog.

ASK – State the key question or the key problem in the investigation. The Point or Purpose of the Experiment.

IMAGINE – Brainstorm solutions for the problem; form a Hypothesis; make a Claim

PLAN – Draw a diagram of the experiment or model; list Materials (use metric units); list a Method (Procedure)

 CREATE – Run Trials (tests); Record Data on Graphs, Tables or Charts; Data must be measurable

IMPROVE – Changes made to the Materials or Method or experimental set-up; run extra trials. May re-visit any of the previous steps.

SHARE & COMMUNICATE – talk and listen to other groups; talk /listen to your teammate; talk about Data/Results; ………. note how science concepts relate to data