Matter and Energy Chapter 1: Introduction to Matter Matter Volume - - PDF document

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Matter and Energy Chapter 1: Introduction to Matter Matter Volume - - PDF document

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Matter and Energy Notes.notebook Matter and Energy Chapter 1: Introduction to Matter Matter Volume Mass Weight Atom Molecule Element Compound Mixture States of Matter Solid Liquid Gas 1 Matter and Energy Notes.notebook Matter and

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Matter and Energy Chapter 1: Introduction to Matter

Matter Volume Mass Weight Atom Molecule Element Compound Mixture States of Matter Solid Liquid Gas

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Matter and Energy Chapter 1: Introduction to Matter

I.Matter has MASS and VOLUME

  • a. Matter is anything that has

mass and takes up space (volume)

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Matter and Energy Chapter 1: Introduction to Matter

Matter is made of up of tiny particles called ATOMS

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Matter and Energy Chapter 1: Introduction to Matter

Everything in the universe is either MATTER OR ENERGY For example light does not have MASS or take up space (VOLUME) Therefore light is energy!

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Matter and Energy Chapter 1: Introduction to Matter

Matter comes in 4 major forms: SOLIDS, LIQUIDS, GASSES, and PLASMAS

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Matter and Energy Chapter 1: Introduction to Matter

MASS is a measure of the amount of matter a substance contains.

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Matter and Energy Chapter 1: Introduction to Matter

The standard unit for mass is the Kilogram (Kg). You would use a TRIPLE BEAM BALANCE to measure mass WEIGHT IS NOT mass!!!!!!!

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Matter and Energy Chapter 1: Introduction to Matter

Weight is the force of gravity on an object. Gravity is the force that pulls 2

  • bjects toward each other.
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Matter and Energy Chapter 1: Introduction to Matter

The standard unit for weight for is NEWTONS (N) A common unit for weight is POUNDS (lbs). You use a SCALE to measure weight

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Matter and Energy Chapter 1: Introduction to Matter

Volume is THE AMOUNT OF SPACE AN OBJECT TAKES UP

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Matter and Energy Chapter 1: Introduction to Matter

Calculating the Volume of an object: Formula: Volume of a rectangle Volume = Length X Width X Height Volume = cm X cm X cm = cm 3

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Matter and Energy Chapter 1: Introduction to Matter

Example: What is the volume of a pizza box that is 8cm high, 38 cm wide and 38 cm long?

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Matter and Energy Chapter 1: Introduction to Matter

Look at the box in the picture below and determine its volume:

SHOW ALL WORK

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Matter and Energy Chapter 1: Introduction to Matter

Measuring Volume by Displacement: Often objects are not a regular shape where volume can be easily calculated using a formula. Instead you can use the displacement method

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Matter and Energy Chapter 1: Introduction to Matter Step 1: Put water into a graduated cylinder and write down the volume: Step 2: Slow and carefully slide the object you want to measure into the graduated cylinder. Step 3: Read the new volume on the graduated cylinder. Step 4: Subtract the volume of the water before from the volume of the water after you added the object.

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Matter and Energy Chapter 1: Introduction to Matter

What is the Volume of the Blue Man?

show work

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Matter and Energy Chapter 1: Introduction to Matter

What is the Density of the Blue Man?

show work

Mass: 2grams

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Matter and Energy Chapter 1: Introduction to Matter

What is the Density of the Dinosaur?

show work

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Matter and Energy Chapter 1: Introduction to Matter

What is the Density of the Dinosaur?

show work

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A cork and a pebble are each placed in 100mL of water, and each displaces 10mL of water. The cork floats, but the pebble sinks. How do the volumes of the cork and the pebble compare?

  • a. They have same volume

b.The cork’s volume is greater c.The pebbles volume is greater d.The volumes cannot be compared using this method

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MATTER IS MADE OF ATOMS

  • a. An atom is the basic unit of

all matter.

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b.Example: Humans are a collection of atoms; a chair is a collection of atoms.

  • c. Atoms are so small that a single

teaspoon of water contains approximately 500,000,000,000,000,000,000,000 atoms.

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  • d. Atoms may be small but they do have

MASS and are in constant MOTION.

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  • e. Atoms are made of 3 even smaller particles

called:

  • i. PROTONS ­ (+) positive charge, and located

in the nucleus.

  • ii. NUETRONS ­ (no) neutral charge, located

in the nucleus.

  • iii. Electrons ­ (e­) negative charge, no mass,

fly around nucleus.

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  • f. A

molecule is formed when 2 or more atoms are bonded together.

  • i. molecules can be made of

atoms that are alike of different

  • ii. Different types of atoms make

up ELEMENTS

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  • iii. WATER

for examples is made up of different kinds of atoms.

  • 1. H2O = 2 Hydrogen atoms and

1 Oxygen atom

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Different molecules can be made up of different amounts of atoms creating different substances (we call these compounds)............

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CO2 = Carbon Dioxide SUBSCRIPTS:The small number in the bottom right corner tells you the number

  • f atoms of the element

before it. When there is no number it means there is

  • nly 1 atom.
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  • 1. CO2 = Carbon Dioxide

a._____ atom(s) of ______________________ _____ atom(s) of _______________________ b.Total number of atoms = ____________

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  • 1. CO2 = Carbon Dioxide

a.1 atom(s) of Carbon 2 atom(s) of Oxygen b.Total number of atoms = 3

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  • 2. CO = Carbon Monoxide

a._____ atom(s) of ______________________ _____ atom(s) of _______________________ b.Total number of atoms = ____________

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  • 2. CO = Carbon Monoxide
  • a. 1 atom(s) of Carbon

1 atom(s) of Oxygen b.Total number of atoms = 2

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  • 3. C6H12O6 = Glucose (Sugar)

a._____ atom(s) of ______________________ _____ atom(s) of _______________________ _____ atom(s) of ______________________ b.Total number of atoms = ____________ ++++

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  • 3. C6H12O6 = Glucose (Sugar)
  • a. 6 atom(s) of Carbon

12 atom(s) of Hydrogen 6 atom(s) of Oxygen b.Total number of atoms = 24

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  • 4. O3 = OZONE!

a._____ atom(s) of ______________

  • b. Total number of atoms = ____________
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  • 4. O3 = OZONE!

a.3 atom(s) of Oxygen

  • b. Total number of atoms =

3

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  • 5. H2SO4

a._____ atom(s) of ______________________ _____ atom(s) of _______________________ _____ atom(s) of ______________________ b.Total number of atoms = ____________

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  • 5. H2SO4

a.2 atom(s) of Hydrogen 1 atom(s) of Sulfur 4 atom(s) of Oxygen b.Total number of atoms = 7

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  • 6. HCl ‐ Hydrochloric Acid

a._____ atom(s) of ______________________ _____ atom(s) of _______________________ b.Total number of atoms = ____________

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  • 6. HCl ‐ Hydrochloric Acid

a.1 atom(s) of Hydrogen 1 atom(s) of Chlorine b.Total number of atoms = 2

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1.3: MATTER COMBINES TO FORM DIFFERENT SUBSTANCES

PURE SUBSTANCE: has only one

  • component. Elements or Compounds only!

Ex: pure water - only water, no minerals or other chemicals

MIXTURES: more than one substance in the same place at the same time but not bonded

  • together. Can be separated easily
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Pure Substances are Atoms, Elements, and Compounds Examples: C = Carbon (element 1 atom) CO2 = Carbon Dioxide: Compound

(2 or more atoms bonded together)

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ATOMS determine the type of substance

Ex - a bar of pure gold, is made up of identical "gold" atoms

ELEMENTS: a type of pure substance that contains only one type of atoms

All the elements are organized on the periodic table on the last page of the chemical interactions text book

PURE SUBSTANCES ARE.........

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COMPOUND: substance that consists of 2 or more different types of atoms (elements) bonded together.

EXAMPLES: H20, HCl, H2SO4, NaCl, H2O2

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MIXTURE: combination of different substances that remain the same individual substances and can be separated physically. Substances are not Bonded!!!

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MIXTURES

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COMPOUNDS vs. MIXTURES

  • 1. Atoms are Bonded

together

  • 2. Can not be

separated physically

  • 3. The properties of a

compound are the same throughout the compound

  • 4. The type and

number of atoms is always the same

  • 1. Materials not

bonded

  • 2. Can be separate

physically

  • 3. Properties change

based on substance.

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Mixtures Heterogenous vs. Homogenous

Can see the individual parts

Cannot see the

  • parts. Looks the

same throughout.

SALT WATER

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Matter Exists in Different Physical States (PHASES)

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Matter Exists in different physical states

  • a. Particle movement and distance

determine the state of matter.....

  • i. When a substance changes from
  • ne form to another, the

arrangement of its molecules changes, the distance between molecules and the attraction between molecules changes.

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Matter Exists in different physical states

SOLID: ­ Fixed (doesn't change) volume ­ Fixed shape ­ Rigid: particles are close together and stay in one place.

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Matter Exists in different physical states

LIQUID: ­ Fixed volume ­ No fixed shaped: takes shape

  • f container

­ Particles not fixed: particles are close together but are free to move around

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Matter Exists in different physical states GAS: ­ NO FIXED VOLUME ­ NO FIXED SHAPE take shape

  • f container

­ Particles are very far apart.

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Matter Exists in different physical states

GAS LIQUID

Evaporation Condensation Freezing

Melting

SOLID

increase in energy(heat) decrease in (energy) heat

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GAS BEHAVIOR:

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GAS BEHAVIOR! Pressure and Volume

When you increase the pressure on a gas, the volume decreases When you decrease the pressure on a gas, the volume increase.

P P

V

V

(inverse proportion)

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GAS BEHAVIOR:

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GAS BEHAVIOR:

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GAS BEHAVIOR: Temperature and Volume:

As the temperature of a gas increases, the volume of the gas increases. As the temperature of the gas decreases, the volume of the gas decreases.

T V T V

(direct proportion)

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GAS BEHAVIOR:

Temperature and Volume:

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GAS BEHAVIOR: