Chemical Bonding

- Negatively Charged - Consists of electrons - Stopped by Aluminum foil - Expressed as 0/-1 e or ß - Very small mass

Beta Particles

What is the formula for iron (III) oxide?

Fe2O3

A positively or negatively charged particle

Ion

- Transfer of Electrons - Between a metal and a nonmetal - Ex: NaCl - Most are brittle - High melting point - All are solids - Form a "crystal lattice" - Good conductors of electric current when dissolved in water.

Ionic Bonds

Left side of the Periodic Table

Metals

Write the chemical formula for sodium oxide.

Na2O

Which element is NOT part of the compound NH4NO3? A. hydrogen B. nickel C. nitrogen D. oxygen

Nickel

Which elements are least likely to react with other elements?

Noble Gases

Right side of the Periodic Table plus hydrogen

Nonmetals

- Number of electrons an atom will gain or lose to become stable - Code: +1, +2, +3, ±4, -3, -2, -1, 0

Oxidation Number

Shows an elements combining ability

Oxidation Number

- Acid—no change - Base—turns Blue

Red Litmus Paper

- A reaction in which one element trades places with another element in a compound - Element and Compound 🡪 - Element and Compound - Dating: CHEATING

Single Replacement Reaction

- The number of electrons on the last energy level - Code: 1, 2, 3, 4, 5, 6, 7, 8

Valence Electrons

Why balance equations?

- The Law of Conservation of Matter Matter is neither created nor destroyed Start = Finish

What is the name of CuO?

Copper (II) Oxide

Write the chemical name for Cu(ClO3)2.

Copper(II) chlorate

- Reaction absorbs energy from its surrounding - Surrounding becomes cooler

Endothermic

A chemical bond between oppositely charged ions

Ionic Bond

Write the chemical name for Fe2s3.

Iron (III) sulfide

HCl is slowly added to aqueous Na2CO3 forming NaCl, H2O, and CO2. Follow the steps above to write a balanced equation for this reaction.

Na2CO3 +2HCl → 2NaCl +H2O +Co2

What kind of chemical reaction involves one substance losing an electron and another substance gaining an electron?

Redox

- Production of a GAS Fizzing, bubbling - Formation of a Precipitate Insoluble solid - Energy is released Light, heat - Color Change

Signs of a Reaction

Which of these is an example of a covalent compound? A. sodium chloride B. calcium fluoride C. calcium chloride D. sulfur dioxide

Sulfur Dioxide

- 4 Main Types: Synthesis, Decomposition, Single Replacement, and Double Replacement - 2 Special Types: Combustion Reaction and Neutralization Reaction

Types of Reactions

A compound composed of two elements

Binary Compound

Write the chemical formula for calcium carbonate.

CaCO3

Write the chemical name for Ca(PO4)2.

Calcium Phosphate

Write the chemical formula for copper sulfate.

CuSO4

- Where two different compounds exchange positive ions (cations) to form two new compounds - All compounds (4 of them) - Dating: Swingers

Double Replacement Reaction

Is the time required for half of a sample to decay

Half—Life

What is the formula for lead (IV) phosphide?

Pb3P4

What is the chemical formula for lead (II) oxide?

PbO

Oxygen gas is always written as O2 in chemical equations. What term is used to describe the "2" in this formula?

Subscript

- When 2 or more substances react to form a single substance - 2🡪1 - Dating: Becoming a Couple

Synthesis Reaction

How do you show that a substance is dissolved in water when writing an equation?

(aq)

How do you indicate that a substance in an equation is a solid?

(s)

What is the oxidation number of of sodium in the compound Na3PO4?

+1

How to Determine If A Compound is an Acid or Base?

- ACID's Formula starts with "H" - BASE's Formula end in "OH" - If it does neither then it is a SALT

How Do I Balance an Equation?

- Id the elements present - Count the amount of atoms on both sides of the "🡪" for each element - Place coefficients in front of compounds and multiply to any subscript - Recount the atoms on both sides of the "🡪" to see if they are equal. If not equal, adjust the coefficients

When 46 g of sodium were exposed to dry air, 62 g of sodium oxide formed. How many grams of oxygen from the air were used?

16 g

Balance this equation: NaOH(aq) + CaBr2(aq) →Ca(OH)2(s) + NaBr(aq).

2NaOH + CaBr2 →Ca(OH)2 + 2NaBr

What is the oxidation number of Fe in the compound Fe2S3?

3+

Chromium is produced by reaching its oxide with aluminum. If 76 g of Cr2O and 27g of Al completely react to form 51 g of Al2O3, how many grams of Cr are formed?

52 g

How many electrons are in the outer energy level of Group 17 elements?

7

When an is chemically stable, how many electrons are in its outer energy level?

8

- Sour Taste - Reacts violently with metals - Electrolyte - Burns the skin - Strong Acids: have high conductivity, high rate of reaction w/ metals and carbonates and a relatively low pH - Weak Acids: have low conductivity, a lower rate of reaction w/ active metals and carbonates and a relatively higher pH

Acid Properties

- Compounds that produces hydronium (H+) ions when dissolved in water - Formula start with "H"

Acids

- Where there is a release of alpha particles - Product has 2 less protons and 2 less neutrons - Mass Number decreases by 4 - Atomic Number decreases by 2

Alpha Decay

- Positively charged - Composed of 2 Protons and Neutrons - Stopped by a thin sheet of paper - Expressed as 4/2 He or α - Has a mass of 4 amu

Alpha Particles

Write the chemical name for (NH4)2SO4.

Ammonium sulfate

- Bitter Taste - Slippery Feel - Will burn the skin - Strong bases - have a high electrical conductivity, fast reaction rate and a very high pH (>>7) - Weak bases - have a low electrical conductivity, slower reaction rate and a pH closer to, but

Base Properties

- Compound that produces hydroxide (OH--) ions when dissolved in water - Formula ends in "OH"

Bases

- Where a neutron decomposes to a proton and electron - Proton Stays - Electron is released - Mass number stays the same - Atomic Number increases by one

Beta Decay

- Acid—turns Red - Base—no change

Blue Litmus Paper

- Is the force that holds atoms or ions together - Three Types Ionic Covalent Metallic

Chemical Bond

- Is a representation of a chemical reaction - Two Parts Reactants Products

Chemical Equation

Tells which elements are in a compound and their ratios

Chemical Formula

When 2 or more elements chemically combine to form a "new" substance

Chemical Reactions

What term is used to describe the "4" in the expression 4Ca(NO3)2?

Coefficient

- When a hydrocarbon (hydrogen and carbon together) reacts with Oxygen - Products are always CO2 & H2O - Ex: CH4 + 2O2 🡪 CO2 + H2O

Combustion Reaction

- Hydrochloric Acid—HCl - Sulfuric Acid—H2SO4 - Nitric Acid—HNO3 - Citric Acid—C6H8O7 - Acetic Acid—CH3COOH

Common Acids

- Calcium Hydroxide—Ca(OH)2 - Magnesium Hydroxide—Mg(OH)2 - Sodium Hydroxide--NaOH

Common Bases

Write the name of the positive ion in the compound. In CuCl, the name of the positive ion is copper.

Copper (I) Chloride

- Number in front is called a coefficient - Coefficients are multiplied to all elements behind it - Subscripts go to what they just follow

Counting Atoms

A bond formed from shared electrons

Covalent Bond

- Sharing of electrons - Between a nonmetal and another nonmetal - Ex: CO2

Covalent Bonds

- When a compound breaks down into two or more substances - 1🡪2 - Dating: Breaking Up

Decomposition Reaction

- Atoms of the same element bonding together - AKA: Super Seven - All are Covalent Bonds

Diatomic Atoms/Molecules

- Atoms of the same element bonding together - AKA: Super Seven - All are Covalent Bonds - F2 - Cl2 - Br2 - I2 - H2 - O2 - N2

Diatomic Atoms/Molecules

- Reaction releases energy to the surrounding - Surrounding becomes warmer

Exothermic

- Splitting the nucleus into two nuclei with smaller masses - Occurs in large mass elements - Produces energy

Fission

- Process where 2 nuclei combine to form a larger mass - Occurs in small mass nuclei - Produces energy (like in the sun, stars, and plasma)

Fusion

- A charged particle - Cations: positive charged ion "+" oxidation number Left Symbol - Anions: negative charged ion "—" oxidation number Right Symbol

Ions

Write the chemical formula for potassium chloride.

KCl

- Sharing of electrons - Between a metal and another metal - Ex: Alloys

Metallic Bonds

Ionic bonds generally form between which two groups of the periodic table?

Metals and nonmetals

A particle made of covalently bonded atoms

Molecule

What must an element be in order to replace another element in a compound?

More reactive

Which of the following formulas represents a nonpolar molecule? A. N2 B. H2O C .NaCl D. HCl

N2

Which is a binary ionic compound? A. O2 B.NaF C. H2SO4 D. Cu(NO3)2

NaF

- 2 elements both being nonmetals Steps 1. Name the first elements 2. Name the second element 3. Change the ending of the second element to "—ide" 4. Add prefixes based on the subscript of each element 5. Place together

Naming Covalent Binary Compounds

- 2 elements present 1 metal then 1 nonmetal Steps 1. Write the name of the first element 2. Write the name of the second element 3. Change the ending of the second element to "—ide" 4. Combine together

Naming Ionic Binary Compounds

- 3 or more elements together Steps 1. Identify the Polyatomic Ion 2. Write the name of the first element 3. Write the name of the polyatomic ions 4. Place together Note: Never change the ending to Polyatomic Ions

Naming Polyatomic Compounds

Which of the following is an atom that has gained an electron? A. negative ion B. positive ion C. polar molecule D. nonpolar molecule

Negative Ion

- When a reaction between an ACID and a BASE produced A SALT and WATER - A Double Replacement Reaction HCl + NaOH 🡪 NaCl + H2O

Neutralization Reaction

What type of bonding occurs between two nitrogen atoms?

Nonpolar Covalent

- Is charged particles and energy that are emitted from the nuclei of radioactive isotopes - Three Types: Alpha, Beta, Gamma

Nuclear Radiation

- Acid—stays clear - Base—turns hot pink

Phenolphthalein

A molecule with partially charged areas

Polar Molecule

A charged group of atoms

Polyatomic Ion

- A group of atoms that acts as a single charged unit - They are covalent Bonds - Ex: PO4—3

Polyatomic Ions

What is the name of KC2H3O2?

Potassium Acetate

- The new substance(s) that form - All things on the right side of the "🡪"

Products

When hydrogen burns, what is oxygen's role?

Reactant

- The substance(s) that undergo the change - All things on the left side of the "🡪"

Reactants

Steps 1. Write the symbols 2. Write the oxidation numbers above the symbols 3. See if the oxidation numbers add to equal zero If it equals ZERO 4a. Write the symbols next to each other If it does not equals ZERO 4b. Cross the oxidation numbers and write as subscripts on the opposite symbol (drop the "+" and "—") Special Notes - If a two or three is being applied to a polyatomic ion, parenthesis goes around the polyatomic ion and the subscript outside of it

Writing Chemical Formulas

- Acid—turns red, orange, yellow tints - Base—turns blue-green to dark blue tints

pH Paper

- Used to determine how acidic or basic something is - From 0—14 (number line) - Acid Range: 0—6 - Strong Acid: 0—2 - Base Range: 8—14 - Strong Base: 10—14 - Water has a pH of 7 (neutral)

pH Scale