Balancing Equations
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The document discusses balancing chemical equations by ensuring that the number of each type of atom is equal on both sides of the reaction arrow. It provides examples of chemical equations and how to balance them by inspecting the numbers of each element in the reactants and products and adjusting coefficients as needed so the numbers are the same on both sides. The document also provides additional examples of chemical equations to balance.
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The document discusses techniques for writing and balancing chemical equations, including representing molecules with chemical formulas, determining the number of atoms in different compounds, using conservation of mass to balance equations, and examples of balancing a variety of chemical reactions. It provides guidance on balancing a number of sample equations involving different elements and compounds.
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The document discusses techniques for writing and balancing chemical equations, including representing molecules with chemical formulas, determining the number of atoms in different compounds, using conservation of mass to balance equations, and predicting and balancing example chemical reactions through inspection of elements on each side of the equation. It provides a number of example chemical equations and reactions to illustrate these concepts.
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This document summarizes different types of chemical reactions:
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2) Synthesis reactions combine two or more substances to form a single product compound.
3) Decomposition reactions involve a single reactant breaking down into simpler substances.
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The document discusses balancing chemical equations by ensuring that the same number and type of atoms appear on both sides of the reaction arrow. It provides examples of balancing a variety of chemical equations involving reactants like Mg, HCl, SO2, and products like MgCl2, SO3, NO2. Students are encouraged to practice balancing many different types of equations involving metals, nonmetals, acids, bases, and other chemicals.
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1. The document defines key chemistry terms including: aqueous solutions, solvents, solutes, electrolytes, nonelectrolytes, strong/weak electrolytes, and solvation.
2. Precipitation reactions are defined as reactions where an insoluble product called a precipitate forms. Molecular, complete ionic, spectator ions, and net ionic equations are also defined.
3. Strong acids and bases are listed as well as examples of soluble and insoluble compounds in water. Spectator ions are identified for sample precipitation reactions.
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The document contains questions about chemistry concepts including:
1) Writing balanced molecular and net ionic equations for neutralization reactions between acids and bases.
2) Defining oxidation, reduction, concentration, molarity, and indicators.
3) Asking if oxidation can occur without accompanying reduction.
4) Calculating oxidation numbers of elements in compounds.
5) Identifying redox, precipitation, and acid-base reactions based on balanced equations.
6) Calculating molarity, moles of solute, and volumes of solutions.
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1. When ions dissolve in water, they are surrounded by water molecules (hydrated).
2. Precipitation will occur when Na2CO3 and AgNO3 or FeSO4 and Pb(NO3)2 are mixed, but not NaNO3 and NiSO4.
3. Acids donate H+ ions, bases accept H+ ions. A monoprotic acid has one ionizable H, a diprotic acid has two. Strong acids fully ionize, weak acids only partially ionize.
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This document provides sample chemistry problems and questions related to topics like:
- Writing balanced equations for neutralization reactions
- Defining terms like oxidation, reduction, concentration, and indicators
- Determining oxidation states of elements in compounds
- Identifying redox, precipitation, and acid-base reactions
- Performing calculations involving molarity, moles, and concentration
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The document discusses balancing chemical equations by ensuring that the same number and type of atoms appear on both sides of the reaction arrow. It provides examples of balancing a variety of chemical equations involving reactants like Mg, HCl, SO2, and products like MgCl2, SO3, NO2. Students are encouraged to practice balancing many different types of equations involving metals, nonmetals, acids, bases, and other chemicals.
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1. The document defines key chemistry terms including: aqueous solutions, solvents, solutes, electrolytes, nonelectrolytes, strong/weak electrolytes, and solvation.
2. Precipitation reactions are defined as reactions where an insoluble product called a precipitate forms. Molecular, complete ionic, spectator ions, and net ionic equations are also defined.
3. Strong acids and bases are listed as well as examples of soluble and insoluble compounds in water. Spectator ions are identified for sample precipitation reactions.
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The document contains questions about chemistry concepts including:
1) Writing balanced molecular and net ionic equations for neutralization reactions between acids and bases.
2) Defining oxidation, reduction, concentration, molarity, and indicators.
3) Asking if oxidation can occur without accompanying reduction.
4) Calculating oxidation numbers of elements in compounds.
5) Identifying redox, precipitation, and acid-base reactions based on balanced equations.
6) Calculating molarity, moles of solute, and volumes of solutions.
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1. When ions dissolve in water, they are surrounded by water molecules (hydrated).
2. Precipitation will occur when Na2CO3 and AgNO3 or FeSO4 and Pb(NO3)2 are mixed, but not NaNO3 and NiSO4.
3. Acids donate H+ ions, bases accept H+ ions. A monoprotic acid has one ionizable H, a diprotic acid has two. Strong acids fully ionize, weak acids only partially ionize.
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This document provides sample chemistry problems and questions related to topics like:
- Writing balanced equations for neutralization reactions
- Defining terms like oxidation, reduction, concentration, and indicators
- Determining oxidation states of elements in compounds
- Identifying redox, precipitation, and acid-base reactions
- Performing calculations involving molarity, moles, and concentration
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The document discusses different types of chemical reactions including synthesis, decomposition, single replacement, double replacement, and combustion reactions. It provides examples of each type of reaction and how to write and balance chemical equations to properly represent these reactions. Key aspects covered include reactants and products, word equations, chemical formulas and symbols, and balancing equations so the number of atoms of each element are equal on both sides.
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This chapter discusses different types of chemical reactions in aqueous solutions. It introduces driving forces that cause reactions, such as formation of a solid, water, or gas. It explains how to predict products using solubility rules and oxidation-reduction reactions when metals react with nonmetals. Reactions are classified into double displacement, acid-base, single replacement, combustion, synthesis, or decomposition reactions based on their driving forces.
SHS STEM General Chemistry MCT 4. Stoichiometry
https://www.deped.gov.ph/wp-content/uploads/2019/01/General-Chemistry-1-and-2.pdf
General Chemistry
GenChem
STEM
Science, Technology, Engineering, and Mathematics
K to 12 Senior High School STEM Specialized Subject – General Chemistry 1 and 2
Quarter 1 – General Chemistry 1
Matter and Its Properties
Measurements
Atoms, Molecules and Ions
Stoichiometry
Percent Composition and Chemical Formulas
Chemical reactions and chemical equations
Mass Relationships in Chemical Reactions
Gases
Dalton’s Law of partial pressures
Gas stoichiometry
Kinetic molecular theory of gases
Quarter 2 – General Chemistry 1
Electronic Structure of Atoms
Electronic Structure and Periodicity
Chemical Bonding
Organic compounds
Quarter 3 – General Chemistry 2
Intermolecular Forces and Liquids and Solids
Physical Properties of Solutions
Thermochemistry
Chemical Kinetics
Quarter 4 – General Chemistry 2
Chemical Thermodynamics
Chemical Equilibrium
Acid-Base Equilibria and Salt Equilibria
Electrochemistry
Chemical Reactions Review (H) Key
The document reviews chemical reactions including synthesis and decomposition reactions, single and double replacement reactions, and examples of writing balanced chemical equations. It provides 11 examples of chemical equations to balance. The document covers key concepts in chemical reactions such as reactants and products, coefficients, states of matter, and conservation of mass.
Chem 1010 Name__________________________________Unit 4-5 Tes.docx
Chem 1010 Name__________________________________
Unit 4-5 Test
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) When the following equation is balanced, the coefficient of Al is __________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
A) 4
B) 1
C) 3
D) 5
E) 2
2) When the following equation is balanced, the coefficient of NaOH is __________.
H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)
A) 1
B) 4
C) 2
D) 0
E) 3
3) When the following equation is balanced, the coefficient of O2 is __________.
C2H4O (g) + O2 (g) → CO2 (g) + H2O (g)
A) 5
B) 3
C) 4
D) 2
E) 1
4) When the following equation is balanced, the coefficient of C3H8O3 is __________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)
A) 2
B) 5
C) 7
D) 1
E) 3
1
5) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium
phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq)
B) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq)
C) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq)
D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)
E) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq)
6) When the reaction shown is correctly balanced, the coefficients are:
C6H6 (l) + O2 (g) → CO2 (g) + H2O (g)
A) 1, 3.5, 6, 7
B) 2, 16.5, 12, 7
C) 2, 15, 12, 6
D) 1, 9.5, 6, 7
E) 1, 6, 6, 7
7) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.
A) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)
B) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g)
C) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
D) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
E) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
8) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
A) H+ and OH-
B) Mg2+ and H+
C) H+ and Cl-
D) OH- only
E) Mg2+ and Cl-
9) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is
________.
A) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)
B) Ag+ (aq) + I- (aq) → AgI (s)
C) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)
D) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)
E) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
10) A neutralization reaction between an acid and a metal hydroxide produces ________.
A) oxygen gas
B) sodium hydroxide
C) ammonia
D) water and a salt
E) hydrogen gas
2
11) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
B) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)
C) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
E) H+ (aq) + OH- (aq) → H2O (l)
12) Which of the following is an oxidation-reduction reaction?
A) Pb(C2H3O2)2(aq) + 2 NaCl(.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Periodic Properties Of Elements In The Periodic Table
The document summarizes periodic properties of elements in the periodic table, including periodic trends in atomic radius, ionization energy, electronegativity, and melting points. It also discusses periodic trends in chemical properties such as formulas of hydrides, oxides, and chlorides as well as their hydrolytic behaviors.
Balance
This document contains a chemistry assignment with multiple parts. It begins with 15 chemical equations to balance. Then it provides an equation for lithium nitride reacting with water and asks 5 questions about mole ratios and amounts needed to produce certain amounts of products. Next is another equation to balance and 6 additional questions about amounts needed to produce an amount of one product. Finally, there are answers provided to balance the initial 15 equations and to the other questions asked.
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Chem 1010 Name__________________________________Unit 4-5 Tes.docx
Chem 1010 Name__________________________________Unit 4-5 Tes.docx
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
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Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
Periodic Properties Of Elements In The Periodic Table
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