Chemical Bonds and Equations

Chemical Bonds and Equations

Types of Chemical Bonds
Compound – substance made of the combined atoms of two or more elements Chemical Formula – tells what elements a compound contains and the exact number of the atoms of those elements Some Common Compounds Vinegar Acetic acid HC2H3O2 Sand Silicon dioxide SiO2 Stomach Acid Hydrochloric acid HCl Cane Sugar Sucrose C12H22O8 Superscript – represents the oxidation # or how many electrons have been gained or lost Coefficient – represents the # of units of each substance 2H2O SO42- Subscript – represents the # of atoms in a molecule of a particular element

Types of Chemical Bonds
Atoms form compounds to become chemically stable. An atom is chemically stable when the outer energy level is complete, or full. Chemical Bond – force that holds together the atoms in a substance. Ionic Bond Loses or gains electrons Attraction between opposite charges of ions Between metal and nonmetal Covalent Bond Shares electrons Can form multiple bonds Between a nonmetal and a nonmetal *Ion – positively or negatively charged atom

Check Quiz on Types of Chemical Bonds

Force

Force atoms

Force atoms more stable

Force Ionic atoms more stable

Force Ionic lost or gained atoms more stable

Force Ionic lost or gained atoms metal and nonmetal more stable

Force Ionic Covalent lost or gained atoms metal and nonmetal more stable

Force Ionic Covalent lost or gained shared atoms metal and nonmetal more stable

Force Ionic Covalent lost or gained shared atoms metal and nonmetal nonmetal and nonmetal more stable

Writing Formulas and Naming Compounds
Binary Compound – compound composed of two elements Oxidation Number – positive or negative number (on Periodic Table) that indicates how many electrons an element has gained, lost or shared when bonding with another atom *When writing formulas for binary ionic compounds, it is important to remember that compounds formed have a net charge of zero Polyatomic Ions Charge Name Formula 1+ Ammonium NH4+ 1- Acetate C2H3O2- Chlorate ClO3- Hydroxide OH- Nitrate NO3- 2- Carbonate CO32- Sulfate SO42- 3- Phosphate PO43- Polyatomic Ions – a positively or negatively charged covalently bonded group of atoms *The prefix poly- means “many”, so the term polyatomic means “having many atoms”

Writing Formulas and Naming Compounds
Hydrate – a compound that has water chemically attached to its ions and written into its chemical formula Covalent compounds can form more than one compound with each other Scientists use Greek prefixes to indicate the # of atoms of each element in a binary compound Prefixes for Binary Covalent Compounds # atoms 1 2 3 4 5 6 7 8 prefix mono- di- tri- tetra penta hexa hepta octa

Writing Formulas: Practice Problems:
Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________ NaCl

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________ NaCl ZnS

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________ NaCl ZnS Zn(OH)2

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________ NaCl ZnS Zn(OH)2 AlCl3

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________ NaCl ZnS Zn(OH)2 AlCl3 K3(PO)4

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl _____________________________ NaCl ZnS Zn(OH)2 AlCl3 K3(PO)4 Pb2O4  PbO2 (reduced)

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- _____________________________ NaCl ZnS Zn(OH)2 AlCl3 K3(PO)4 Pb2O4  PbO2 (reduced) MnBr4

Step 1: Write the symbol of the element or the polyatomic ion that has the positive oxidation number (hydrogen, ammonium ion (NH4+) and all metals) Step 2: Write the symbol of the element or polyatomic ion with the negative oxidation number (nonmetals and polyatomic ions other than NH4+) Step 3: Add subscripts so that the sum of the oxidation numbers of all atoms in the formula is zero – use crisscross method: The charge (without the sign) of one ion becomes the subscript of the other ion Examples: Na+, Cl- ______________________________ Zn2+, S2- ______________________________ Zn2+, OH- _____________________________ Al3+, Cl- ______________________________ K+, PO43- _____________________________ Pb4+, O2- _____________________________ Mn4+, Br- _____________________________ H+, Cl- ______________________________ NaCl ZnS Zn(OH)2 AlCl3 K3(PO)4 Pb2O4  PbO2 (reduced) MnBr4 HCl

Naming Compounds: Step 1: Write the name of the first element
*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Calcium carbonate Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Calcium carbonate Sulfur dioxide Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Calcium carbonate Sulfur dioxide Phosphorus tribromide Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Calcium carbonate Sulfur dioxide Phosphorus tribromide Magnesium nitrite Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Calcium carbonate Sulfur dioxide Phosphorus tribromide Magnesium nitrite (Di)phosphorus pentoxide Check Quiz on Writing Formulas and Naming Compounds

*Note – subscripts do not become part of the name for ionic compounds but are used to determine prefixes when naming covalent compounds Step 2: Write the root of the name of the second element Ex.: Chlorine root is chlor-, Oxygen root is ox-, and Bromine root is brom- Step 3: Add the ending –ide to the root Ex.: (Ionic) BaF2 – Barium Fluoride; AlCl3 – Aluminum Chloride Ex.: (Covalent) N2O – dinitrogen monoxide; CO – carbon monoxide; CO2 – carbon dioxide Sulfur hexachloride Silicon dioxide Calcium carbonate Sulfur dioxide Phosphorus tribromide Magnesium nitrite (Di)phosphorus pentoxide Check Quiz on Writing Formulas and Naming Compounds Carbon tetrachloride

Chemical Reactions Chemical Reaction – a reaction in which one or more substances are changed to new substances Reactants – substances that are about to react Products – new substances produced Law of Conservation of Mass – total starting mass of all reactant equals the total final mass of all products Chemical Equation – uses chemical formulas and symbols to describe a chemical reaction and the product it produces (see below) Symbol Meaning produces or yields plus (s) solid (l) liquid (g) gas Symbol Meaning (aq) Aqueous (solid dissolved in H2O) Heat Reactants heated Light Reactants exposed to light Electricity Electric current applied to reactant *Review: Coefficients - #s that represent the number of units of each substance in a reaction 4Al (s) + 3O2 (g)  2Al2O3 Subscripts - #s that represent the number of atoms in a molecule of a particular element

Coefficients

Subscript Coefficients

Subscript Coefficients Reactants

Subscript Coefficients Products Reactants

Produces / Yields Subscript Coefficients Products Reactants

Produces / Yields Subscript Coefficients Products Reactants Solid

Produces / Yields Aqueous Subscript Coefficients Products Reactants Solid

Produces / Yields Aqueous Subscript Coefficients Products Reactants Solid Gas

MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s)
Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: Equation B: 2. What are the products in: 3. What do the coefficients tell you about the ratio of the reactants in: 4. What is the physical state of the products in: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: 2. What are the products in: Equation A: 3. What do the coefficients tell you about the ratio of the reactants in: 4. What is the physical state of the products in: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: Equation B: 3. What do the coefficients tell you about the ratio of the reactants in: 4. What is the physical state of the products in: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: 4. What is the physical state of the products in: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: NaCl and Mg 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: Equation B: 4. What is the physical state of the products in: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: NaCl and Mg 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: 2:1 Equation B: 4. What is the physical state of the products in: Equation A: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: NaCl and Mg 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: 2:1 Equation B: 1:2 4. What is the physical state of the products in: Equation A: Equation B: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: NaCl and Mg 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: 2:1 Equation B: 1:2 4. What is the physical state of the products in: Equation A: liquid Equation B: 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: NaCl and Mg 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: 2:1 Equation B: 1:2 4. What is the physical state of the products in: Equation A: liquid Equation B: aqueous and solid 5. Write Equation A as a sentence. Check Quiz on Chemical Reactions

Equation A Equation B 2H2(g) + O2(g)  2H2O (l) MgCl2(aq) + 2Na(s)  2NaCl(aq) + Mg(s) 1. What are the reactants in: Equation A: H2 and O2 Equation B: MgCl2 and Na 2. What are the products in: Equation A: H2O Equation B: NaCl and Mg 3. What do the coefficients tell you about the ratio of the reactants in: Equation A: 2:1 Equation B: 1:2 4. What is the physical state of the products in: Equation A: liquid Equation B: aqueous and solid 5. Write Equation A as a sentence. Two units of hydrogen (gas) combined with one unit of gaseous oxygen produce two units of liquid water. Check Quiz on Chemical Reactions

Balancing Chemical Equations
Steps to Balancing a Chemical Equation: Balancing Chemical Equations Step 1: Write a chemical equation for the reaction using formulas and symbols – make sure reactants are on left side and products on right side. Step 2: Count the atoms in reactants and products. Step 3: Choose coefficients that balance the equation. Hint: Generally, if there is an even # of an element on one side and an odd on the other side, place a 2 in front of compound containing odd number of atoms. Step 4: Recheck the numbers of each atom on both sides of equation and adjust coefficients if necessary – remember, NEVER change subscripts. Balanced chemical equations – have the same number of atoms of each element on both sides of equation *When balancing chemical equations, NEVER change the subscripts – instead, change the coefficient in front of the compounds needing balanced

Balancing Chemical Reactions
Check Quiz on Balancing Chemical Equations Balancing Equation Practice Worksheet

Chemical Reactions – Types, Rates and Energy
Synthesis Reaction – reaction where two or more substances combine to form another substance A + B  AB Decomposition Reaction – reaction where one substance breaks down, or decomposes, into two or more simpler substances AB  A + B Singe-displacement Reaction – reaction in which one element replaces another in a compound A + BC  AC + B or A + BC  AB + C Double-displacement Reaction – reaction that results in a precipitate, water or gas when a positive ion of one compound swaps with another positive ion of another compound AB + CD  AC + BD

Types of Reactions Practice Problems:
N2 + 3H2  2NH3

Decomposition N2 + 3H2  2NH3

Decomposition Synthesis N2 + 3H2  2NH3

Decomposition Synthesis Single Displacement N2 + 3H2  2NH3

Decomposition Synthesis Single Displacement Decomposition N2 + 3H2  2NH3

Decomposition Synthesis Single Displacement Decomposition Synthesis N2 + 3H2  2NH3

Decomposition Synthesis Synthesis Single Displacement Decomposition Synthesis N2 + 3H2  2NH3

Decomposition Synthesis Synthesis Single Displacement Single Displacement Decomposition Synthesis N2 + 3H2  2NH3

Decomposition Synthesis Synthesis Single Displacement Single Displacement Single Displacement Decomposition Synthesis N2 + 3H2  2NH3

Decomposition Synthesis Synthesis Single Displacement Single Displacement Single Displacement Decomposition Synthesis Synthesis N2 + 3H2  2NH3

Decomposition Synthesis Synthesis Single Displacement Single Displacement Single Displacement Decomposition Synthesis Synthesis N2 + 3H2  2NH3 Double Displacement

Chemical Reactions – Types, Rates and Energy
Chemical Reactions involve energy exchange Exothermic Reactions Reaction in which energy is released in form of heat Ex.: burning wood, fireworks explode Endothermic Reactions Reaction in which heat energy is absorbed Ex.: chemical ice packs, photosynthesis Catalyst – speeds up a chemical reaction without itself being permanently changed Inhibitor – prevents or slows a chemical reaction or interferes with the catalyst Check Quiz on Types of Chemical Bonds

Chemical Bonds and Equations

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