crhs academic chemistry unit 1 matter and change notes 1 matter... · crhs academic chemistry unit...

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CRHS Academic Chemistry

Unit 1 Matter and Change Notes

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1.1 MATTER

Definition - Matter is anything that has MASS and takes up SPACE

Chemistry is the science that describes matter, how it changes, and how those changes affect energy. To start, how do we classify matter? By their states (or phases)!

THE STATES (or phases) OF MATTER

Shape? Volume?

Particle Arrangement?

Effect of change in pressure?

Solid

Definite Shape

Definite Volume

Tightly packed particles (moving!) No change

Liq

uid

NO Definite Shape

Definite Volume

(takes shape of container)

Closely packed, but particles glide over one another.

Very Little change

Gas

NO Definite Shape

NO Definite Volume

(fills container)

Loosely arranged particles travel randomly through the container.

Significant amount of change

OK, but WHAT is matter?

ALL matter is composed of _____________ of chemical elements

An atom is one type of particle in chemistry, and is the smallest unit of an element.

Mass is the amount of ____________________ the object contains.

Regardless of state, ALL MATTER can be divided into ____ groups: P_____ S______________ and M _________

Unit 1 Notes of 12

1. Pure Substances – have a constant composition throughout the sample; contain only ONE type of matter.

o Element – the ____________________ form of matter and are made of only _________ type of atom.

The PERIODIC TABLE lists all known elements. Flerovium (114) and Livermorium (116) were added in

2013. Division of the parts of an element is called a nuclear reaction, a topic for another day.

o Compound – _________ or more elements bound together. Can be divided into simpler substances

only by a chemical reaction (Example: MgCO3 decomposes into MgO and CO2)

2. Mixtures – a physical blend of substances. Contains more than one type of matter; composition may vary.

Can almost always be separated by physical means. Iced tea, ocean water, sand, and steel are examples.

o Homogeneous – appears ____________________ (uniform) throughout. A homogenous mixture

containing a liquid is called a solution (Ex. Salted water)

o Heterogeneous – DO NOT appear uniform. We can easily see different parts of the mixture. (Ex.

_______________________)

Mg - CO2 -

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Chemical vs. Physical Properties

A “Property” is a CHARACTERISTIC of a pure substance. They can either be physical or chemical.

1. Physical property – can be observed or measured BUT DOES NOT CHANGE the identity of a material.

a. ________________ property – depends on the AMOUNT of matter present (mass, length, heat, volume) b. _______________ property – does NOT depend on the amount of matter present (density, specific heat, melting point, phase)

EXTENSIVE Depends on AMOUNT of matter

INTENSIVE Does NOT depend on amount of matter

Mass

Volume

Length

Density

Color

Melting Point

Pure Substances Mixtures

MATTER

Unit 1 Notes of 12

Practice: Label property as Intensive (I) or Extensive (E) Blue Color ____ Mass ____Volume ____ Temperature ____ Boiling Point ____ Hardness ____ Density ____

2. Chemical property – ability of a substance to undergo a change that changes the identity of the

substance.

Examples: ______________________________________

*Turn to pages 11 to look for properties of hydrochloric acid (HCl) in the Material Safety Data Sheet. MSDS

are available for all chemicals in the lab both in our MSDS binder AND online!

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1.2 DENSITY

Density is an intensive property of pure substances that is a ratio of the mass of an object relative to the

volume of the same object.

𝐷𝑒𝑛𝑠𝑖𝑡𝑦 =𝑀𝑎𝑠𝑠

𝑉𝑜𝑙𝑢𝑚𝑒 𝑑 =

𝑚

𝑣

Units: MASS is measured in metric unit grams (g)

VOLUME is based in either:

i. milliliters (mL)

ii. cubic centimeters (cm3)

1 mL = 1 cm3

Density will be expressed in g/mL OR g/cm3

Example: What is the density of a 114 g mass of lead that has a volume of 10.0 cm3?

𝑑 = 𝑚

𝑣

The density of water at room temperature is 1.00 g/cm3. Therefore…

Anything with a density_________ than 1.00 g/cm3 will sink in water (Density > water)

Anything with a density _________ than 1.00 g/cm3 will float in water (Density < water)

Example: A cube of ice has a mass of 5 g and a volume of 10 cm3. Will this ice cube float in a glass of

water?

𝑑 = 𝑚

𝑣

Unit 1 Notes of 12

Practice: You have a 23.0-g sample of ethanol with a density of 0.7893 g/ml. What volume of ethanol

do you have?

Practice: The density of aluminum is 2.7 g/mL. How much mass is there in a 3.0 mL sample of

aluminum?

Practice: A piece of metal with a mass of 147 g is placed in a graduated cylinder. The water level rises from 20.0 mL to 41.0 mL. What is the density of the metal?

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1.3 PHYSICAL vs CHEMICAL “CHANGE” & CONSERVATION OF MASS

Physical change – alters a material without changing its identity.

Examples: ___________ change (melting, freezing, sublimating, evaporating, condensing), cutting,

breaking, separating, dissolving

Phase Change Diagram

(Physical Change)

Chemical change – any change in which pure substances are converted into different pure substances with

different characteristic properties. A chemical change means a chemical reaction has occurred.

Examples: ______________________________________

Chemical reactions are accurate and balanced representations of the events of chemical change. We write

them like this:

REACTANT(S) PRODUCT(S)

Reactants – Substances that begin a chemical reaction; written on the LEFT side of the arrow

Products – Substances produced by a chemical reaction; written on the RIGHT side of the arrow

Melting

Boiling

Thermal Energy Increases

Temperature

Increases

Unit 1 Notes of 12

Examples of Chemical Reactions (We study the types of chemical reactions in Unit 8)

2H2 + O2 2H2O

2NaCl 2Na + Cl2

2 Li + MgBr2 Mg + 2 LiBr

FOUR Indicators of a chemical change/reaction

1. ___________ exchange (temperature change, emission of light)

2. Change in _________________

3. Production of _______________ (odor, bubbles)

4. Formation of a precipitate

Precipitate: an insoluble product of a chemical reaction. Usually a solid.

Practice: Label the examples below as physical or chemical changes.

a. _____________Iron rusting

b. _____________Glass breaking

c. _____________Rubbing alcohol catches fire

d. _____________Polar ice cap melts

e. _____________Glucose dissolving in water

f. _____________Bathroom cleaner on lime scale creates small bubbles and the lime scale breaks

down

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Law of the Conservation of Mass

Law of Conservation of Mass in words – Matter cannot be created or destroyed

Law of Conservation of Mass as a formula – In a chemical reaction, the mass of the reactants ______________

the mass of the products.

Example: Consider the chemical reaction in which carbon reacts with oxygen to produce carbon dioxide.

What mass of carbon dioxide would be produced if 20.1 grams of carbon reacted completely with 62.5

grams of oxygen?

C + O2 CO2

20.1 g 62.5 g ? The Conservation of Mass law tells us that the total mass on both sides must be equal, so… 20.1 g + 62.5 g = 82.6 g

Practice: When ammonium nitrate (NH4NO3) breaks down explosively, it forms nitrogen gas (N2), oxygen

gas (O2), and water(H2O). When 38 grams of ammonium nitrate explode, 13 grams of nitrogen and 7

grams of oxygen are formed. How many grams of water are formed?

NH4NO3 N2 + O2 + H2O

Practice: Methane (natural gas) is reacted with oxygen in residential furnaces to generate heat during

colder months. The same reaction is used in our laboratory as a common heat source. It takes 500 g of

oxygen to burn 125g of methane completely generating 281 g of water. What mass of carbon dioxide was

also generated?

CH4 + 2O2 CO2 + 2H2O + Heat

Unit 1 Notes of 12

Material Safety Data Sheet (MSDS) 395.10

SECTION 1 — CHEMICAL PRODUCT / COMPANY IDENTIFICATION

Hydrochloric Acid

Flinn Scientific, Inc. P.O. Box 219 Batavia, IL 60510 (800) 452-1261

SECTION 2 — COMPOSITION, INFORMATION ON INGREDIENTS Hydrochloric acid (7647-01-0)

Synonyms: muriatic acid, toilet bowl cleaners, tile cleaners

CAS# - None established

SECTION 3 — HAZARDS IDENTIFICATION Clear acidic solution. Pungent chlorine odor. Toxic by inhalation and ingestion. Severely corrosive to all body tissues, especially skin and eyes.

Avoid all body contact. Health-2, Flammability-0, Reactivity-2, Exposure-3, Storage-3. 0 is low hazard, 3 is high hazard

SECTION 4 — FIRST AID MEASURES Call a physician and seek medical attention for further treatment, observation, and support after first aid. Inhalation: Remove to fresh air at once. If

breathing has stopped, give artificial respiration immediately. Eye: Immediately flush with fresh water for at least 15 minutes. External: Wash

continuously with fresh water for at least 15 minutes. Internal: Give large quantities of water or milk, followed by a gastric antacid, such as milk of

magnesia. Do not induce vomiting. Call a physician or poison control at once.

SECTION 5 — FIRE FIGHTING MEASURES Nonflammable liquid. When heated to decomposition, emits toxic fumes of HCl and Cl2 or explosive H2 gas. Fire Fighting Instructions: Use a

triclass, dry chemical fire extinguisher. Firefighters should wear PPE and SCBA with full facepiece operated in positive pressure mode.

NFPA CODE: None established.

SECTION 6 — ACCIDENTAL RELEASE MEASURES Restrict unprotected personnel from the area. Remove all ignition sources and ventilate area. Contain the spill with sand or other inert absorbent

material, neutralize with sodium bicarbonate or calcium hydroxide, and deposit in a sealed bag or container. See Sections 8 and 13 for further

information.

SECTION 7 — HANDLING AND STORAGE Flinn Suggested Chemical Storage Pattern: Inorganic #9. Store with inorganic acids.

Store in a dedicated acid cabinet and away from any source of water; if an acid cabinet is not available, store in Flinn Saf-Cube. Use and dispense in

a hood or in a well-ventilated lab only.

SECTION 8 — EXPOSURE CONTROLS, PERSONAL PROTECTION Avoid contact with eyes, skin, and clothing. Wear chemical splash goggles, chemical-resistant gloves, and chemical-resistant apron. Use ventilation

to keep airborne concentrations below exposure limits. Always wear a NIOSH-approved respirator with proper cartridges or a positive pressure, air-

supplied respirator when handling this material in emergency situations (spill or fire).

SECTION 9 — PHYSICAL AND CHEMICAL PROPERTIES Clear fuming liquid with a pungent odor.

Solubility: Soluble in water and alcohol.

Formula: HCl Formula Weight: 36.46 pH < 1

SECTION 10 — STABILITY AND REACTIVITY Avoid contact with (Reacts violently with) strong oxidizers, bases, metals, metal oxides, hydroxides, amines, and other alkaline materials.

Incompatible with cyanides, sulfides, and formaldehyde. Corrodes metal, including steel. Produces heat and may splatter violently when diluted with

water. Shelf Life: Good, if stored safely.

SECTION 11 — TOXICOLOGICAL INFORMATION Acute effects: Poison, corrosive. Chronic effects: Corrosive to teeth. Target organs: Respiratory tract, teeth, skin

SECTION 12 — ECOLOGICAL INFORMATION Does not biodegrade in soil, may be toxic to aquatic life.

SECTION 13 — DISPOSAL CONSIDERATIONS Please consult with state and local regulations. Flinn Suggested Disposal Method #24b is an option.

SECTION 14 — TRANSPORT INFORMATION Shipping Name: Hydrochloric acid

Hazard Class: 8, Corrosive

UN Number: UN1789

SECTION 15 — REGULATORY INFORMATION TSCA-listed, EINECS-listed (231-595-7), RCRA code D002

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