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
SHS STEM General Chemistry MCT 6. Electronic Structure of AtomsEngineerPH EducatorPH
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
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
Stoichiometry deals with the numerical relationships of elements and compounds and the mathematical proportions of reactants and products in chemical transformations
SHS STEM General Chemistry MCT 6. Electronic Structure of AtomsEngineerPH EducatorPH
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
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
Stoichiometry deals with the numerical relationships of elements and compounds and the mathematical proportions of reactants and products in chemical transformations
Structural diagrams,condensed structures and line structures of hydrocarbons.How to identify a substance as Organic and inorganic ?.How to classify hydrocarbons? What is the difference between alkanes,alkenes and alkynes?
This power point work describe about polar and nonn polar compounds and how to find it very easily and it also explain dipole moment and its calculation...this includes some workout problems
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
Organic compounds are almost 60% of all compounds. because of carbons tendency to form a compound as it has more than1 electron(4electrons) to form covallent compounds. SO a wide range of everything we eat is formed from carbon and hydrogen, which is the second important element to form organic compounds.
CHEMICAL REACTION
CHEMICAL EQUATION
CHEMICAL FORMULA
BALANCING
TYPES OF CHEMICAL REACTION
COLLISION THEORY
FACTORS AFFECTING THE RATE OF CHEMICAL REACTION
Structural diagrams,condensed structures and line structures of hydrocarbons.How to identify a substance as Organic and inorganic ?.How to classify hydrocarbons? What is the difference between alkanes,alkenes and alkynes?
This power point work describe about polar and nonn polar compounds and how to find it very easily and it also explain dipole moment and its calculation...this includes some workout problems
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
Organic compounds are almost 60% of all compounds. because of carbons tendency to form a compound as it has more than1 electron(4electrons) to form covallent compounds. SO a wide range of everything we eat is formed from carbon and hydrogen, which is the second important element to form organic compounds.
CHEMICAL REACTION
CHEMICAL EQUATION
CHEMICAL FORMULA
BALANCING
TYPES OF CHEMICAL REACTION
COLLISION THEORY
FACTORS AFFECTING THE RATE OF CHEMICAL REACTION
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(.
Chapter 4 Problems1. Which of these compounds is a strong elec.docxketurahhazelhurst
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of ...
Chapter 4 Problems1. Which of these compounds is a strong elec.docxrobertad6
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of.
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DepEd SHS STEM General Chemistry Modules Quarters 1-2 by Tapayan
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
K to 12 SENIOR HIGH SCHOOL (STEM) Curriculum Guide in General Chemistry (with...EngineerPH EducatorPH
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
Most Essential Learning Competencies (MELC) in Senior High School (STEM) Gene...EngineerPH EducatorPH
General Physics
GenPhy
STEM
Science, Technology, Engineering, and Mathematics
K to 12 Senior High School STEM Specialized Subject – General Physics 1 and 2
General Physics 1:Units and Measurement Vectors
Kinematics
Newton’s Laws
Work and Energy
Center of Mass, Momentum, Impulse and Collisions
Rotational Equilibrium and Rotational DynamicsGravity
Periodic Motion
Mechanical Waves and Sounds
Fluid Mechanics
Temperature and Heat
Ideal Gases and Laws of Thermodynamics
General Physics 2:
Electricity and Magnetism
Optics
Modern Physics Concepts
Most Essential Learning Competencies (MELC) in Senior High School (STEM) Gene...EngineerPH EducatorPH
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
Most Essential Learning Competencies (MELC) in Senior High School (STEM) Gene...EngineerPH EducatorPH
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
SHS STEM General Chemistry 2 Study Notes in Chemical Equilibrium (Problem Set) EngineerPH EducatorPH
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
K-12 Most Essential Learning Competencies (MELC) Grades 1-10 and SHS CoreEngineerPH EducatorPH
DepEd Science Grade 3 DepEd Science Grade 4 DepEd Science Grade 5 DepEd Science Grade 6
DepEd Science Grade 7
DepEd Science Grade 8
DepEd Science Grade 9
DepEd Science Grade 1
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
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
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
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
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
For more information, visit-www.vavaclasses.com
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Palestine last event orientationfvgnh .pptxRaedMohamed3
An EFL lesson about the current events in Palestine. It is intended to be for intermediate students who wish to increase their listening skills through a short lesson in power point.
Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
Acetabularia Information For Class 9 .docxvaibhavrinwa19
Acetabularia acetabulum is a single-celled green alga that in its vegetative state is morphologically differentiated into a basal rhizoid and an axially elongated stalk, which bears whorls of branching hairs. The single diploid nucleus resides in the rhizoid.
1. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
Choose the letter of the correct answer. Write your answer on the space provided
before each number.
___1. Calculate the number of molecules in a spoonful of table sugar
(C12H22O11) having a mass of 10.5g.
A. 6.29 × 1024
B. 1.13 × 1023
C. 1.85 × 1022
D. 3.01 × 1023
___2. Calculate the mass in grams of a sample containing 1.85 × 1034
molecules of water.
A. 3.07 × 1010 g
B. 5.53 × 1011 g
C. 188 g
D. 8.46 × 103 g
___3. Which of the following is NOT an empirical formula?
A. NO2
B. H2N
C. CH
D. C3H6
___4. What is the empirical formula of a compound with the molecular formula
C8H16 and a molecular weight of 112.21 amu?
A. C8H16
B. C2H4
C. CH3
D. CH2
2. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
___5. Calculate the mass of 0.333 mol CO2. The molar mass of carbon dioxide
is 44.0 g.
A. 120 g
B. 12.5 g
C. 13.3 g
D. 14.7 g
___6. Calculate the percentage by mass of nitrogen in HNO3.
A. 22.2 percent
B. 20.0 percent
C. 25.0 percent
D. 76.2 percent
___7. Three common ways of measuring the amount of something are by count,
by mass, and by
A. temperature.
B. volume.
C. area.
D. density.
___8. The atomic mass of fluorine is 19.0 amu, so the molar mass is
A. 19.0 amu.
B. 19.0 g.
C. 6.02 × 1023 amu.
D. 6.02 × 1023 g.
___10. Calculate the percentage by mass of carbon in cadaverine, C5H14N2, a
compound present in rotting meat.
A. 67.4 percent C
B. 58.8 percent C
C. 51.7 percent C
D. 68.2 percent C
3. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
___11. Balance the following equation.
Al + Cr2O3 → Al2O3 + Cr
A. 2Al + Cr2O3 → Al2O3 + 2Cr
B. 2Al + Cr2O3 → Al2O3 + Cr
C. 4Al + 2Cr2O3 → 2Al2O3 + 4Cr
D. Al + Cr2O3 → Al2O3 + 2Cr
___12. Identify the correct net ionic equation for the following reaction and the
spectator ion, if there is one.
FeO(s) + 2HClO4(aq) → H2O(l) + Fe(ClO4)2(aq)
A. FeO(s) + 2H+(aq) + 2ClO4
-(aq) → H2O(l) + Fe2+(aq) + 2ClO4
-(aq); no
spectator ion
B. FeO(s) + 2H+(aq) + 2ClO4
-(aq) → H2O(l) + Fe2+(aq) + 2ClO4
-(aq); ClO4- is a
spectator ion.
C. FeO(s) + 2H+(aq) → H2O(l) + Fe2+(aq); ClO4
- is a spectator ion.
D. FeO(s) + 2HClO4(aq) → H2O(l) + Fe(ClO4)2(aq); no spectator ion
___13. Balance the following equation and indicate whether it represents a
combustion, combination, or decomposition reaction.
H2SO4 → H2O2 + SO2
A. H2SO4 → H2O2 + SO2, combination reaction
B. H2SO4 → H2O2 + SO2, decomposition reaction
C. H2SO4 → 2H2O2 + SO2, combination reaction
D. H2SO4 → 2H2O2 + SO2, decomposition reaction
___14. What coefficient is needed for HCl when the following equation is
correctly balanced?
CaCO3(s) + HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
A. 1
B. 2
C. 3
D. 4
4. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
___15. What is(are) the spectator ion(s) when a BaCl2 solution is combined with
an H2SO4 solution?
A. Ba2+(aq), H+(aq)
B. SO4
2-(aq), H+(aq)
C. Cl-(aq)
D. Cl-(aq), H+(aq)
___16. Which of the following is a skeleton equation?
A. H2 + CO → CH3OH
B. 2H2 + CO → CH3OH
C. 2H2 + CO2 → CH3OH
D. hydrogen + carbon monoxide → methanol
___17. Choose the correct net ionic equation for the reaction that occurs when
the following compounds are mixed: AgNO3(aq) and Na2CO3(aq).
A. 2AgNO3(aq) + Na2CO2(aq) → Ag2CO3(s) + 2NaNO3(aq)
B. 2Na+(aq) + 2NO3(aq) → 2NaNO3(s)
C. 2Ag+(aq) + CO32-(aq) → Ag2CO3(s)
D. 2Na+(aq) + 2Ag+(aq) + 2NO3
-(aq) + CO3
2-(aq) → Ag2CO3(s) + 2NaNO3(s)
___18. Which one of the following substances should be soluble in water?
A. AgCl
B. PbSO4
C. Mg(OH)2
D. Mo(NO3)2
___19. Choose the correct equation for the reaction of hydrobromic acid with
zinc.
A. Zn(s) + HBr(aq) → ZnBr(aq) + H+(aq)
B. Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g)
C. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
D. Zn(s) + 2HBr(aq) → ZnBr(aq) + H2(g)
5. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
___20. What is the net ionic equation for the reaction between aqueous Sr(OH)2
and FeSO4 solutions?
A. Sr2+(aq) + SO4
2-(aq) → SrSO4(s).
B. Fe2+(aq) + 2OH-(aq) → Fe(OH)2(s).
C. Fe2+(aq) + SO4
2-(aq) → FeSO4(s).
D. Sr2+(aq) + SO4
2-(aq) + Fe2+(aq) + 2OH(aq) → SrSO4(s) + Fe(OH)2(s).
___21. The alcohol in gasohol burns according to the following equation.
C2H5OH + 3O2 → 2CO2 + 3H2O.
How many moles of CO2 are produced when 3.00 mol of C2H5OH are burned
in this way?
A. 3.00 mol
B. 6.00 mol
C. 2.00 mol
D. 4.00 mol
___22. Automotive airbags inflate when sodium azide, NaN3, rapidly
decomposes to its component elements via this reaction.
2NaN3 → 2Na + 3N2
How many grams of sodium azide are required to form 5.00 g of nitrogen
gas?
A. 9.11 g
B. 8.81 g
C. 7.74 g
D. 3.33 g
___23. Choose the correct values for the spaces. 27.0 g H2O are formed from
24.0 g O2 and __________ g H2. The same 24.0 g O2 could form __________
grams of H2O2 if there were sufficient H2.
A. 3.0, 28.0
B. 3.0, 25.5
C. 6.0, 28.0
D. 48.0, 25.5
6. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
___24. If 3.00 mol of gaseous SO2 react with oxygen to produce sulfur trioxide,
how many moles of oxygen are needed?
A. 3.00 mol O2
B. 6.00 mol O2
C. 1.50 mol O2
D. 4.00 mol O2
___25. How many grams of iron oxide, Fe2O3, can be produced from 2.50 g of
oxygen reacting with solid iron, according to the following equation?
2Fe(s) + 3O2(g) → Fe2O3(s)
A. 12.5 g
B. 8.32 g
C. 2.50 g
D. 11.2 g
___26. Octane burns according to the following equation.
2C8H18 + 25O2 → 16CO2 + 18H2O
What is the percent yield if 14.6 g of CO2 are produced when 5.00 g of C8H18
are burned?
A. 106%
B. 94.8%
C. 34.2%
D. 62.5%
___27. Silicon carbide, SiC, is commonly known as carborundum. This hard
substance, which is used commercially as an abrasive, is made by heating
SiO2 and C to high temperatures.
SiO2(s) + 3C(s) → SiC(s) + 2CO(g)
How many grams of SiC form when 3.00 g of SiO2 and 4.50 g of C are
allowed to react?
A. 2.00 g
B. 3.00 g
C. 5.01 g
D. 15.0 g
7. Quarter I General Chemistry 1
Stoichiometry
STEM_GC11S-Ie-(25to30); STEM_GC11PCIf-(31to33);
STEM_GC11CRIf-g-(34to37); STEM_GC11MRIg-h-(38to42)
Multiple-Choice Test
___28. The total mass of all reactants in a chemical reaction
A. cannot be determined.
B. equals the mass of the products.
C. is less than the products.
D. is more than the products.
___29. How many moles of water are produced when 2.5 mol of O2 react
according to the following equation?
C3H8 + 5O2 → 3CO2 + 4H2O
A. 4.0
B. 3.0
C. 2.5
D. 2.0
___30. A reaction that produces iron metal from iron ore is shown below.
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)
How many moles of iron are produced from the reaction of 10 mol Fe2O3 and
25 mol of CO?
A. 10 mol
B. 17 mol
C. 25 mol
D. 35 mol