Chapter 11 Section 2 Page 287 - The Atom & Subatomic Particles

  • The atom is ______(has no overall charge) because there are equal numbers of protons and electrons (See chart below)
  • SEE DIAGRAM – The atom is composed of ______(C), neutrons (A), & ______(D).
  • The ______(B) of the atom is composed of protons & neutrons.
  • The energy levels (orbits) of an atom are composed of electrons______. Valence electrons are in the ______ENERGY LEVEL & are responsible for bonding because they have the most energy.
  • The smallest particle of protons & neutrons are ______.
  • Size of order from least to greatest part of an atom is the ______, quark, ______, and nucleus.

Name of Element / Protons
Atomic Number / Neutrons
(atomic mass minus atomic number) / Electrons
  1. Neon
/ 10 / 10 / 10
  1. Calcium
/ 20 / 20 / 20

Chapter 12 – Arranging the Elements –Periodic Table of the Elements Pages 304 – 317

Metals, Nonmetals and Metalloids (page 306-307)

Metals, Nonmetals & Metalloids

Most periodic tables contain a stairstep line which allows you to identify which elements are metals, nonmetals and metalloids. Following are descriptions of each of the 3 types of materials.

Metals

  • Most elements are metals. 88 elements to the ______of the stairstep line are metals or metal like elements

Physical Properties of Metals:

  • ______(shininess)
  • Good ______of heat and electricity
  • High ______(heavy for their size)
  • High melting point
  • ______(most metals can be drawn out into thin wires)
  • ______(most metals can be hammered into thin sheets)

Chemical Properties of Metals:

  • Easily ______electrons
  • ______easily. Corrosion is a gradual wearing away. (Example: silver tarnishing, iron rusting, and batteries)

NonMetals

______are found to the right of the stairstep line. Their characteristics are opposite those of metals.

Physical Properties of Nonmetals:

  • No luster (dull)
  • ______conductor of heat and electricity
  • Brittle (breaks easy)
  • Not ______
  • Not malleable
  • Low density
  • Low ______point

Chemical Properties of Nonmetals:

  • Tend to ______electrons

Since metals tend to ______electrons and nonmetals tend to ______electrons, metals and nonmetals like to form compounds with each other. These compounds are called ionic compounds. When 2 or more nonmetals bond with each other they form a ______.

Family or Groups and Periods Arrangement (page 309)

Family or ______are columns.(vertical) ______are rows. (horizontal)

Chapter 13 IONIC AND COVALENT BONDS

Section 2 Pages 332-337

Ionic Bonds (Bonding between Metal and Nonmetal)

  • Is the force of attraction between oppositely charged ions (+, -)
  • Ions are charged particles that form during chemical changes when one or more ____________transfer from one atom to another.
  • Example: Lithium Chloride (LiCl)

Lithium (Li) is in group 1 (1 valence electron); therefore transfers 1 valence electron to chlorine. Lithium is a metal and now a positively charged ion. Lithium’s charge is Li+1.

Chlorine (Cl) is in group 17 (7 valence electrons); therefore accepts 1 valence electron from lithium (Li). Chlorine (Cl) is a nonmetal and now is negatively charged ion. Chlorine’s charge is Cl-1.

Covalent Bonds (Bonding between Nonmetal & Nonmetal)

  • Is the force of attraction between the nuclei of atoms and the electrons shared by atoms.
  • Does NOT form bonds that involve ions.
  • Covalent bonds ______valence electrons and form covalent bonds called

______.

Chapter 14 CHEMICAL REACTIONS

FORMING NEW SUBSTANCES

Section 1 Pg. 350 - 357

Chemical Reaction is the process by which one or more substances undergo change to produce one or more different substances.

Clues for Chemical Reactions:

  • Gas bubbles
  • Solid forms in a solution as a result this is called ______.
  • ______change
  • Energy change: ______or stored

Breaking Bonds and Making Bonds

Chemical Formula: is a shorthand notation for a compound or a diatomic element using ______and numbers.

Chemical formula indicates the chemical makeup by showing how many of each kind of atoms is present in a molecule.

______is a number written below and to the right of a chemical symbol in a formula. H2O

Question: How many atoms of each element make up Na2SO4?

(pg. 354) Chemical Equations is a shorthand description of a chemical reaction using chemical formulas & symbols.

Reactants Yield Products USING CARBON AND OXYGEN AS AN EXAMPLE

  • Carbon reacting with Oxygen to yield Carbon Dioxide CO2.
  • Starting material in a chemical reaction are______. (Carbon & Oxygen)
  • Substances formed from a reaction are ______. (Carbon Dioxide CO2)

Reactants Products

C + O2 CO2 + sign separate the formulas of two or more reactants or products from one another

Equations MUST be balanced: When writing a chemical equation, you must show that the number of atoms of each element in the reactants equals the number of atoms of those elements in the products by writing a balanced equation.

LAW OF CONSERVATION OF MASS states that mass is neither ______nor ______in any ordinary chemical reaction. Or more simply, the mass of substances produced (products) by a chemical reaction is always equal to the mass of the reacting substances (reactants). Established in 1789 by French Chemist Antoine Lavoisier.

HOW to BALANCE an EQUATION: Write a balanced equation for H2 + O2 H2O

#1 Count the atoms of each element in the reactants & in H2 + O2 H2O

the products. You can see that there are fewer O Reactants Products

atoms the products than in the reactants.

H = 2 O=2 H = 2 O= 1

#2To balance the O atoms, place the coefficient 2 in H2 + O2 2 H2O

front of water’s formula. This gives you 2 O atoms Reactants Products

in both the reactants & the products. But now there

are too few hydrogen atoms in the reactants.

H= 2 O = 2 H = 4 O = 2

#3To balance the hydrogen atoms, place the coefficient 2H2 + O2 2H2O

2 in front of H’s formula. But just to be sure your Reactants Products

Answer is correct, always double-check your work!

Question: Balancing Act: When balancing a chemical

equation, you must place coefficients in front of an H = 4 O = 2 H = 4 O = 2

entire chemical formula, never in the middle of a

formula. Notice where the coefficients are in the balanced equation below:

F2 + 2KCl 2KF + Cl2

Now it is your turn: Write balanced equations for the following: HCl + Na2S H2S + NaCl

and Al + Cl2 + AlCl3

Questions: 1. How many atoms of each element make up 2Na3PO4?

2. Write the chemical formulas for carbon tetrachloride and calcium bromide.

Sec. 2 pg. 358 - 360

Types of Chemical Reactions

  1. ______Reaction is a reaction in which two or more substances combine to form a single compound.
  • Example: 2 people join together to make a couple or 2Na + Cl2 2NaCl

2.Decomposition Reaction is a reaction in which a single compound breaks down to form two or more simpler substances

  • Decomposition reaction is the ______ of Synthesis Reaction
  • Couple and they break up or H2CO3 H2O + CO2

3. Single-Replacement Reactionis a ______in which an element takes the place of another element that is part of a compound.

  • Zn + 2HCl ZnCl2 + H2
  • More-reactive elements replace less-reactive elements in single-replacement reactions.

4. Double-Replacement Reaction is a reaction in which ions in 2 compounds ______places.

  • One of the products of the reaction is often a gas or a precipitate.
  • Examples: 2 dance couples dancing and then switch partners.
  • NaCl + AgF NaF + AgCl

Questions:

1. What type of reaction does each of the following equations represents?

  1. FeS + 2HCl FeCl2 + H2S
  2. NH4OH NH3 + H2O

2. Which type of reaction always has an element and a compound as reactants?

3. Compare synthesis and decomposition reactions.

ENERGY & RATES OF CHEMICAL REACTIONS

Section 3 Pg. 361 - 364

Exothermic Reactions

  • Exo means “go out” or “______”
  • ______means “heat” or “energy”
  • Energy released in an exothermic reaction is often written as a ______in a chemical equation.

2Na + Cl2 2NaCl + energy

  • Types of energy released in Reactions
  • ______energy – example light sticks
  • ______Energy – example: batteries (dry cells) in a flashlight
  • ______& Thermal Energy – example: campfire

Endothermic Reactions

  • ______means “in”
  • Energy is ______in an endothermic reaction and is often written as a ______in a chemical equation.

2H2O + energy 2H2 + O2

PHOTOSYNTHESIS – ______reaction

  • Endothermic process in which light energy from the sun is used to produce glucose, a simple sugar.
  • MOST IMPORTANT ENDOTHERMIC REACTION carried on by plants and some protest – PHOTOSYNTHESIS
  • Phytoplankton use photosynthesis to produce food.
  • Photosynthesis Equation: THIS WILL BE ON THE SOL

Which is the Reactant? Which is the Products?

6CO2 + 6H2O 6CO2 + 6H2O + energy

  • Cells in your body use glucose to get the energy they need through cellular ______, an “exothermic” process described by the reverse of the above reaction: (see below equation)

C6H12O6 + 6O2 6CO2 + 6H2O + energy

  • Endothermicreactions ______energy and absorbed.
  • ______energyis the minimum amount of energy needed for substances to react.
  • Energy produced during the formation of products is greater than the activation energy…energy is given off.
  • Activation energy required is greater than the energy produced in the reaction …energy is absorbed.

RESPIRATION -______reaction

  • Chemical reactions to living things – extremely important!
  • Provides energythat allows the living organisms to perform all the functions necessary to maintain life.
  • All living ______must carry out cellular respiration.
  • Opposite of photosynthesis: all living things carry out respiration
  • Chemical Equation: Reactions Products
  • 1 molecule of glucose + 6 molecules of O 6 molecules of CO2 + 6 molecules of H2O
  • C6H12O6 + 6O2 6CO2 + 6H2O + energy

Ways to increase the rate of a reaction:

  • ______– rising the temperature
  • ______– increase the amount of reactants (more people more to collide)
  • ______– exposed surface
  • Catalysts & Inhibitors –
  • ______– substance that speeds up a reaction w/o being permanently changed.
  • Examples: enzymes in your body & catalysts in a car
  • ______–substance that slows down or stops a chemical reaction.
  • Examples: preservatives for food & poisons

Questions:

  1. Compare exothermic and endothermic reactions.
  2. Do these energy diagrams show an exothermic or an endothermic reaction?

How can you tell?

a. b.

3. What is activation energy?

4. List 4 ways to increase the rate of a reaction.

LAWOFCONSERVATION OF ENERGY

  • States that energy can be neither created nor destroyed!
  • Energy will be absorbed/stored.
  • Energy will have the same amountbefore and after the reaction.
  • Energy released in ______ reactions arestored in the reactants.
  • Energy ______in endothermic reactions is stored in the ______that form.

Chapter 15 Chemical Compounds pg. 372 - 389

Section 1 – IONIC & COVALENT COMPOUND pg 374-376

Ionic Compoundis the force of attraction between two oppositely charged ions.

  • Formed by the reaction of a metal with a nonmetal.
  • Electrons are ______from the metal atoms (+ ions) to the nonmetal atoms (-ions)

Properties of Ionic Compounds

  • Crystal lattice pattern (positive & negative alternate)
  • Brittle (shatters easily)
  • High ______point: Mg melts @ 2800oC; Nickel oxide melts @ 1984oC; Potassium Dichromate melts @ 398oC
  • ______@ room temperature
  • ______– dissolve in water
  • ______– conduct an electric current

Questions:

1. Where are the metals and nonmetals located on the periodic table?

2. List ALL of the properties of Ionic Compound

3. Ionic Compound’s electrons are ______.

4. What is an Ionic Compound?

Covalent Compoundsare covalent bonds form when atoms SHARE electrons.

  • Examples: gasoline, carbon dioxide, water and sugar

Properties of Covalent Compounds

  • Low melting point
  • ______- independent particles
  • ______- do not dissolve in water
  • ______– does not conduct electricity (including compounds called ACIDS)

Questions:

1. List the properties of Covalent Compounds

2. Methane is a gas at room temperature. What type of compound is this most likely to be?

3. Create Venn diagram using Ionic and Covalent Compounds on the type of particles that make up each.

Section 2 - ACIDS, BASES and SALTS pg. 377 – 382

  • Acidity and basicity are ______properties
  • Acids and bases ______each other
  • Example: Antacids are taken to soothe heartburn by neutralizing hydrochloric acid in the stomach

Properties of Acids

  • Acids are ______, meaning they destroy body tissue and clothing
  • Acids ______electrical current
  • Acids increase the number of hydrogen ions (H+) in a water solution
  • Acids in a water solution each hydrogen ion bonds to a water molecule H2O to form H3O+
  • ______paper detects an acid and staysred
  • Blue Litmus paper detects an ______and turnsred
  • Acids have a sour taste
  • Acids have a pH of 0-6

Uses of Acids

  • Sulfur Acid – Industrial chemicalproduces of metals, paper, paint, detergents & fertilizers
  • Car batteries
  • Nitric acid is used for fertilizers, rubber, & plastics
  • HCl used in metals and keep swimming pools from algae; aids in digestion
  • Citric Acid & Ascorbic acid (Vitamin C) found in Orange Juice

Properties of Bases

  • Bases taste ______
  • Bases are slippery (like soap)
  • Bases ______electrical current
  • Bases increase the number of hydroxide ions (OH-)in a water solution
  • Red Litmus paper detects a ______and turns______blue
  • Blue Litmus paper detects a base and stays blue
  • Bases have a pH of 8-15

Uses of Bases

  • NaOH– (Sodium Hydroxide) makes soap & paper; unclogs drains; oven cleaner
  • CaOH – (Calcium Hydroxide) makes cement, mortar and plaster
  • Ammonia – household cleaners, fertilizers
  • MgOHAlOH - (Magnesium Hydroxide) antacids to treat heartburn

Indicators

  • An indicator is a substance that changes ______in the presence of an acid or base.
  • Blue litmus paper detects an ______and turns red
  • Red litmus paper detects a ______and turns blue
  • In the computer lab exercise and in class lab the indicator was cabbage juice.
  • An acid turned pink, a base green and a neutral substance stayed purple.

pHstands for “______”

0-6 Acids

7-Neutral (Neither Basic or Acidic)

8-14 Bases

Increasing Acidity Neutral Increasing Basicity

1 2 3 4 5 6 7 8 9 10 11 12 13 14

Neutralization Reactions

  • Acids and bases ______one another to create salt and water
  • Acid + Base Salt + Water
  • In the reaction of vinegar and baking soda, the vinegar is an acid and the baking soda is a base. They combine in a chemical reaction to create sodium acetate, water and carbon dioxide.

REACTANTS PRODUCTS

Acid + Base Salt + Water

(H+ ion)(ion-) + (ion+)(OH-ion) Sodium Chloride + Water

HCl + NaOHNaCl + H2O

SALTS – pg 382

Saltis an_____ compound forming from the positive ion of a base and the negative ion of an acid.

  • A Salt & water are produced when an acid neutralizes a base.

Uses of Salts

  • Industries & your home
  • ______your food (table salt)
  • Produces lye, baking soda, HCl, NaOH (sodium hydroxide)
  • Calcium Sulfate – wallboard, plasterboard used in construction
  • Calcium carbonate makes up limestone, chalk, and seashells.
  • ______on roads and bridges

Questions:

1. What ion is present in all acid solution?

2. What are two ways scientist can measure pH?

3. What products are formed when an acid and base react?

4. Compare the properties of acids and bases. Use a Venn diagram.

5. Would you expect the pH of a solution of soap to be 4 or 9 on the pH scale?

6. Is the compound H3PO4 an acid or a base? How do you know?

7. Would you expect the pH of a sample of acid rain to be 4 or 9 on the pH scale? Why?

8. What products would form when hydrochloric acid (HCl), and sodium hydroxide, NaOH, react?

Hydrocarbons

  • Hydrocarbons are compounds that contain ______hydrogen and carbon.
  • Example: Ethane
  • Water and carbon dioxide are produced when ethane is combined with oxygen & burned

2C2H6+ O2 CO2 + 4H2O

Balanced:

2C2H6 + 7O2 4CO2 + 6H2O

Water & potassium chloride are produced when potassium hydroxide & hydrochloric acid react.

HCl + KOH KCl + H2O

Balanced:

HCl + KOH KCl + H2O

When aluminum oxide decomposes, aluminum and oxygen are produced.

Al2O3 Al + O2

Balanced:

2H2O 2H2 + O2

Hydrogen can be produced by passing an electric current through water. Oxygen is also a product of this reaction.

H2O H2 + O2

Balanced:

2H2O 2H2 + O2

When iron is in contact with oxygen, iron oxide is formed.

Fe + O2 Fe2O3

Balanced:

4Fe + 3O2 2Fe2O3

Questions:

1. What is a hydrocarbon?

2. How many electrons are share in a double bond? A triple bond?

3. Compare saturated and unsaturated hydrocarbons. Use a Venn diagram.

Vocabulary: Know these vocabulary words for your Unit Test.

Section 1

  • Ionic compounds - pg 374
  • Covalent compounds -pg 375

Section 2

  • Acid – pg 377
  • Base – pg 379
  • pH – pg 380
  • Salt – pg 382

Section 3

  • Organic compounds – pg 383
  • Biochemical – pg 384
  • Carbohydrates – pg 384
  • Lipids – pg 385
  • Proteins – pg 386
  • Nucleic acids – pg 387
  • Hydrocarbons – pg 388