Garde 11 Stem General Chemistry Module Prelim
Garde 11 Stem General Chemistry Module Prelim
Garde 11 Stem General Chemistry Module Prelim
MODULE 1
General Chemistry
Quarter 1 – Week 1
NAME: __________________________________________
SECTION & GRADE: ________________________________
CONTACT NO.:____________________________________
ADDRESS: ________________________________________
In the name of the Father, and of the Son, and of the Holy
Spirit. Amen.
Our Father, Who art in heaven, hallowed be Thy name; Thy kingdom come; Thy will be
done on earth as it is in heaven. Give us this day our daily bread; and forgive us our
trespasses as we forgive those who trespass against us; and lead us not into
temptation, but deliver us from evil. Amen. In the name of the Father, and of the Son,
Properties of Matter
Most Essential Learning Competencies
Content Standard
The learners demonstrate understanding of the properties of matter and its various
forms.
Performance Standard
The learners should be able to design using multimedia, demonstrations, or
models, a representation or simulation of any of the following:
A. Atomic structure
B. Gas behavior
C. Mass relationships
D. Reactions
PRE-ASSESSMENT
ACTIVITY SHEETS
Matter is anything that takes up space (has a volume) and has a mass. In other
words, everything that makes up our physical and chemical world is matter.
Physical properties are ones that we can observe without chemically changing a
substance. For example, the hardness and color of a substance are both physical
properties. No new substances are formed when we make these observations.
Remember that physical properties can also be either qualitative (such as the colour of
gold being yellow or copper metal being shiny/lustrous) or quantitative (such as the
density of H2O being 1.0 g/cm3 and the melting point of H2O being 0° C).
Chemical properties are properties that can be measured or observed only when
matter undergoes a change to become an entirely different kind of matter. For example,
the ability of iron to rust can only be observed when iron actually rusts. When it does, it
combines with oxygen to become a different substance called iron oxide. Iron is very
hard and silver in color, whereas iron oxide is flakey and reddish brown. Besides the
ability to rust, other chemical properties include reactivity and flammability.
Elements are pure substances that are made up of only one kind of atoms. Possible
examples: iron; gold; mercury.
ELEMENT FORMULA
Iron Fe
Gold Au
mercury Hg
Diatomic Elements (consists of 2 similar atoms)
Hydrogen H2
Oxygen O2
Nitrogen N2
Fluorine F2
Chlorine Cl2
Bromine Br2
Iodine I2
Compounds are pure substances made up of two or more kinds of atoms. Possible
examples: salt; sugar; water
COMPOUND FORMULA
Sodium Chloride (table salt) NaCl
Water H2O
Magnesium Fluoride MgF2
A homogeneous mixture has a uniform composition and exhibits the same properties
in different parts of the mixture. Examples: saltwater, air.
Separation of Mixtures
ACTIVITY SHEETS
Week 1 – Day 2
Pure Substances and Mixtures in Consumer
Products
Most Essential Learning Competencies
Compare consumer products on the basis of their components for use, safety,
quality and cost
PRE-ASSESSMENT
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
List down all the substances found in your kitchen and in the bathroom. The more
answer the better because this will be useful on your next activity! (10 points)
CHAPTER INTRODUCTION
Consumer product, also referred to as final goods, are products that are bought by
individuals or households for personal use.
Bleach
Soaps
Cosmetics
There are many chemical combinations used for the preparation of these cosmetics.
The chemicals added is what gives the texture and feel for these kinds of beauty
products. Cosmetics are made from a range of ingredients which are the so called
industrial chemicals. Industrial chemicals may be either synthetic chemicals or naturally
occurring processed chemicals. Few of the chemicals and its use in the cosmetic are
listed below.
3. Alcohols are common ingredients in perfumes. The fatty alcohols(less dense alcohol
after the removal of fats and oils in alcohols) are ingredients in detergent and act as
cleansing agents. The glycols are used as substances to avoid loss of moisture.
Isopropanol is the common alcohol ingredient in many cosmetics and cleansing
products. Usually used to reduce the thickness of liquid.
4. Lanolin is a thick substance derived from the sebaceous gland of sheep. It is a thick
moisturizing agent. It is a common additive in cosmetic products for moisturizing skin,
hair and nails. This act as an emulsion by blending with any other cosmetic product.
5. Mineral waxes are common ingredient in cosmetics. They are main ingredients in
products such as paraffin oil, paraffin wax, petrolatum (known as Vaseline).
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Using your answer on the pre-assessment activity, classify some substances found in
the kitchen and in the bathroom as pure substances or mixtures; elements or
compounds; and homogeneous or heterogeneous mixture. (15 points)
Content Standard
The learners demonstrate understanding of the properties of matter and its various
forms.
Performance Standard
The learners should be able to design using multimedia, demonstrations, or
models, a representation or simulation of any of the following:
A. Atomic structure
B. Gas behavior
C. Mass relationships
D. Reactions
CHAPTER INTRODUCTION
Videos:
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Activity 5 : DISTILLATION
Observe and think of any natural processes that is similar to distillation that happen in
our surrounding. (5 points each)
Example No. 1
Example No. 2
LICEO DE LOS BAÑOS
M. Palis St. Timugan, Los Baños, Laguna
SY. 2020-2021
Learning Module in
General Chemistry
Quarter 1 – Week 2
NAME: __________________________________________
SECTION & GRADE: ________________________________
CONTACT NO.:____________________________________
ADDRESS: ________________________________________
In the name of the Father, and of the Son, and of the Holy
Spirit. Amen.
Our Father, Who art in heaven, hallowed be Thy name; Thy kingdom come; Thy will be
done on earth as it is in heaven. Give us this day our daily bread; and forgive us our
trespasses as we forgive those who trespass against us; and lead us not into
temptation, but deliver us from evil. Amen. In the name of the Father, and of the Son,
Content Standard
The learners demonstrate understanding of...
1.atomic structure
2. formulas and names of compounds
Performance Standard
The learners should be able to design using multimedia, demonstrations, or
models, a representation or simulation of any of the following:
A. Atomic structure
B. Gas behavior
C. Mass relationships
D. Reactions
Specific Learning Outcomes:
At the end of this lesson, the learners will be able to:
1. define atomic number and mass number;
2. identify common isotopes; and
3. give uses of some isotopes.
PRE-ASSESSMENT
ACTIVITY SHEETS
Matter is composed of atoms, and atoms have three basic building blocks. Label each
part of the atom without looking at your periodic table and from your own idea, give the
definition of each parts. (10 points)
CHAPTER INTRODUCTION
Kindly read Atomic Number, Mass Number and Isotopes on pages 58 to 60 of
General Chemistry 1 (Rex Book Store).
Answer
Isotopes are atoms of an element having the same atomic number but different mass
number. The existence of isotopes was shown by mass spectroscopy experiments,
wherein elements were found to be composed of several types of atoms, each with
different masses.
a. The atomic number identifies an element. The atoms of isotopes of an element have
the same number of protons and electrons.
Carbon is normally present in the atmosphere in the form of gaseous compounds like
carbon dioxide and methane. Carbon-14 (14C) is a naturally occurring radioisotope that
is created from atmospheric 14N (nitrogen) by the addition of a neutron and the loss of
a proton, which is caused by cosmic rays. This is a continuous process so more 14C is
always being created in the atmosphere. Once produced, the 14C often combines with
the oxygen in the atmosphere to form carbon dioxide. Carbon dioxide produced in this
way diffuses in the atmosphere, is dissolved in the ocean, and is incorporated by plants
via photosynthesis. Animals eat the plants and, ultimately, the radiocarbon is distributed
throughout the biosphere.
In living organisms, the relative amount of 14C in their body is approximately equal to
the concentration of 14C in the atmosphere. When an organism dies, it is no longer
ingesting 14C, so the ratio between 14C and 12C will decline as 14C gradually decays
back to 14N. This slow process, which is called beta decay, releases energy through
the emission of electrons from the nucleus or positrons.
Radioactive isotopes find uses in agriculture, food industry, pest control, archeology and
medicine. Radiocarbon dating, which measures the age of carbon-bearing items, uses a
radioactive isotope known as carbon-14. In medicine, gamma rays emitted by
radioactive elements are used to detect tumors inside the human body. Food irradiation
-- the process of exposing food to a controlled level of gamma rays -- kills many types of
bacteria, making food safer to eat.
https://sciencing.com/types-isotopes-uses-8571746.html
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Week 2 – Day 2
Formulas of Compounds
Content Standard
The learners demonstrate understanding of...
1.atomic structure
2. formulas and names of compounds
Performance Standard
The learners should be able to design using multimedia, demonstrations, or
models, a representation or simulation of any of the following:
A. Atomic structure
B. Gas behavior
CHAPTER INTRODUCTION
Chemists use tools to represent the composition of molecules and compounds in terms
of chemical symbols. The composition of a molecule or an ion can be represented by a
chemical formula. The formula consists of the symbols of the atoms making up the
molecule. If there is more than one atom present, a numerical subscript is used.
a. O2 – oxygen gas
b. H2O – water
Molecular formula – gives the composition of the molecule, in terms of the actual
number of atoms present.
i. C6H12O6
ii. K3PO4
iii. Na2C2O4
Empirical formula – gives the composition of the molecule, in terms of the smallest
ratio of the number of atoms present.
i. CH2O
ii. NaCO2
Structural Formula – shows the bond pattern and connectivity of atoms in compounds.
An atom is represented by its element symbol, while lines depict the type of chemical
bond between the atoms. The lines ─, = and ≡ represent single, double and triple bond
respectively.
Table 1. Molecular, Empirical and Structural Formulas of Some Compounds
Kindly read Chemical Formulas on pages 67-68 of General Chemistry 1 (Rex Book
Store).
2. A simple cation (obtained from a single atom) takes its name from the name of the
element.
3. A simple anion (obtained from a single atom) is named by taking the first part of the
element name (the root) and adding the letters “ide.”
4. Write the name for the compound by combining the names of the ions.
O is the symbol for oxygen, whose root is “ox.” Add the “ide” ending to get oxide.
Rules for naming compounds with metals with more than one ion
2. A simple cation (obtained from a single atom) takes its name from the name of the
element. Include a Roman numeral to indicate the oxidation number (charge) on the
metal cation.
3. A simple anion (obtained from a single atom) is named by taking the first part of the
element name (the root) and adding the letters “ide.”
4. Write the name for the compound by combining the names of the ions.
Cl is the chemical symbol for chlorine, whose root is “chlor.” Add the “ide” ending
to get chloride.
Divide the total positive charge by the number of atoms to get Roman numeral.
There is only 1 Fe +2 divided by 1 = +2. The Roman numeral is II.
Put the pieces together to get the name iron (II) chloride.
b. Molecular compounds – made up of two non-metals. They are named by giving
the name of the first nonmetal and then that of the second nonmetal modified by
the ending -ide. Molecular compounds are usually gases.
1. The first element in the formula is named first, and the full element name is used.
3. Prefixes are used to denote the numbers of atoms present. (See table below)
4. The prefix mono- is never used for naming the first element.
N is the chemical symbol of nitrogen. Since there is only one nitrogen atom AND
it is the first element the prefix mono is not used.
is the chemical symbol of oxygen, whose root is ox. Add the ide ending to get
oxide. There are two oxygen atoms so we also add the prefix di to get dioxide.
Put the pieces together to get the name nitrogen dioxide.
Examples:
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Write the formula for the following ionic compounds: (10 points)
a. sodium bicarbonate_________________
b. sodium fluoride _________________
c. iron (III) chloride _________________
d. odium carbonate _________________
e. copper (II) sulfate _________________
f. lithium sulfate _________________
g. magnesium chloride _________________
h. silver nitrate _________________
i. calcium sulfate _________________
j. magnesium iodide _________________
Write the formulas for the following covalent compounds: (9 points)
f. carbon tetrachloride_________________________
g. hydrogen monochloride_________________________
Week 2 – Day 3
Percent Composition and Chemical Formulas
Content Standard
The learners demonstrate understanding of the mole concept in relation to Avogadro’s
number and mass
Performance Standard
The learners should be able to design using multimedia, demonstrations, or
models, a representation or simulation of any of the following:
A. Atomic structure
B. Gas behavior
C. Mass relationships
D. Reactions
2. calculate the empirical formula from the percent composition of a compound; and
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Activity 9
Percentage of the class planning (as first choice) to go to the different strands in STEM.
(12 points)
2. Get the number of learners who would like to pursue engineering in college. Get the
percentage.
3. Get the number of learners who would like to pursue the sciences. Get the
percentage.
4. Get the number of learners who would like to pursue mathematics. Get the
percentage.
Information from the chemical formula
What information can be obtained from a chemical formula? For example, what
information can you get from the formula of carbon dioxide, CO 2?
b. One molecule of CO2 is made up of one atom of carbon and two atoms of oxygen.
c. One mole of CO2 molecules will have one mole of C atoms and two moles of O
atoms.
e. CO2 is composed of 27.29% carbon and 72.71% oxygen. The chemical formula
provides the percent composition of CO2.
For CO2,
The answer indicates that CO2 is composed of 27.29% C atom and 72.71% O atom.
Learning Module in
General Chemistry
Quarter 1 – Week 3
NAME: __________________________________________
SECTION & GRADE: ________________________________
CONTACT NO.:____________________________________
ADDRESS: ________________________________________
PRAYER
In the name of the Father, and of the Son, and of the Holy
Spirit. Amen.
Our Father, Who art in heaven, hallowed be Thy name; Thy kingdom come; Thy will be
done on earth as it is in heaven. Give us this day our daily bread; and forgive us our
trespasses as we forgive those who trespass against us; and lead us not into
temptation, but deliver us from evil. Amen. In the name of the Father, and of the Son,
The empirical formula of a compound can be calculated from the percent composition.
Because percentage is given, it is convenient to assume 100.00 grams of the
compound.
A. A compound is found to consist of 7.81% C and 92.19% Cl. What is the empirical
formula of the compound? Assume 100.00 grams of the compound. The sample
will therefore contain 7.81 g C and 92.19 g Cl. The grams are converted to moles
to get the ratios of the moles of the elements in the compound:
Kindly read and take a look at the examples about calculation of percent
composition and determining chemical formulas on pages 88-92 of General
Chemistry 1 of Rex book Store.
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Activity 10
Content Standard
The learners demonstrate understanding of the use of chemical formulas to
represent chemical reactions
Performance Standard
The learners should be able to design using multimedia, demonstrations, or
models, a representation or simulation of any of the following:
A. Atomic structure
B. Gas behavior
C. Mass relationships
D. Reactions
PRE-ASSESSMENT
Answer Activity 11 on page 39
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Activity 11
We can represent this reaction through a chemical equation. The reactants (starting
substances) are placed on the left side. The products (substances produced) are placed
on the right. An arrow points towards the direction of the reaction. The equation has to
be balanced so that the same number and types of atoms appear on the left and right
side of the equation. To balance, coefficients (numbers preceding the chemical formula)
are used. For additional information, the physical states of the reactants and products
(s, l, g, for solid, liquid, or gas, respectively) are indicated. Hence, the balanced
chemical equation is:
Reactants Products
H=2 H =2
Cl =2 Cl =2
Ethane (C2H6) reacts with oxygen gas (O2) to produce carbon dioxide and water. Write
the balanced chemical equation for the reaction.
1. Identify reactants and products and write their correct formulas. Put reactants on the
left side and products on the right.
ACTIVITY SHEETS
Activity 12
Week 3 – Day 3
Mass Relationships in Chemical Reactions
Most Essential Learning Competencies
Construct mole or mass ratios for a reaction in order to calculate the amount of
reactant needed or amount of product formed in terms of moles or mass
Content Standard
The learners demonstrate understanding of...
CHAPTER INTRODUCTION
a. Determine how much products will be produced from a specific amount of reactants
The balanced equation says that 3 moles H2 are stoichiometrically equivalent to 1 mole
N2 and to 2 moles NH3. The ratio of moles H2 to moles NH3 is 3:2; the ratio of moles
N2 to moles
NH3 is 1:2.
a. How many moles of NH3 will be produced if 10.4 moles H2 react completely with
N2? (moles H2 → moles NH3)
2moles NH 3
10.4 moles H2 x = 6.93 moles NH3
2 moles H 2
b. How many moles of N2 are needed to produce 42.4 moles NH3? (moles NH3 →
moles N2)
1 moles N 2
42.4 moles NH3 x = 21.2 moles N2
2moles NH 3
c. How many grams of NH3 will be produced from 25.7 moles N2 (moles N2 → moles
NH3 → g NH3)
2moles NH 3 17.03 g NH 3
25.7 moles N2 x x = 875 g NH3
1mole N 2 2moles NH 3
d. How many grams of NH3 will be produced if 122 g N2 reacts completely with H2? (g
N2→moles N2 → moles NH3 →g NH3)
Solid lithium hydroxide is used to remove carbon dioxide and is called a CO2
scrubber. This technique has been used for space vehicles. The reaction is:
Stoichiometry https://www.khanacademy.org/science/chemistry/chemical-reactions-
stoichiome/stoichiometry-ideal/a/stoichiometry
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Activity 13
2 H2O → 2 H2 + O2
1. How many moles of O2 are produced when 1.26 moles of H2O is reacted?
2. How many moles of H2O are needed to produce 55.7 moles of H2?
3. If enough H2O is reacted to produce 3.40 moles of H2, then how may moles of
O2 must have been made? (a bit challenging, but just think about it and you can
probably figure it out)
Show your solution:
LICEO DE LOS BAÑOS
M. Palis St. Timugan, Los Baños, Laguna
SY. 2020-2021
Learning Module in
General Chemistry
Quarter 1 – Week 4
NAME: __________________________________________
SECTION & GRADE: ________________________________
CONTACT NO.:____________________________________
ADDRESS: ________________________________________
In the name of the Father, and of the Son, and of the Holy
Spirit. Amen.
Our Father, Who art in heaven, hallowed be Thy name; Thy kingdom come; Thy will be
done on earth as it is in heaven. Give us this day our daily bread; and forgive us our
trespasses as we forgive those who trespass against us; and lead us not into
temptation, but deliver us from evil. Amen. In the name of the Father, and of the Son,
Week 4 – Day 1
Percent Yield and Theoretical Yield
Content Standard
The learners demonstrate understanding of...
Limiting Reagents
The reactant used up first in the chemical reaction is called the limiting reagent. Excess
reagents re reactants present in quantities greater than what is needed by the reaction.
Illustrate using the following examples:
When Karen went shopping, she was able to buy 50 slices of cheese, 20 hamburger
patties, and 50 slices of bread. How many double cheeseburgers can she make? What
is the limiting material or reagent? What are the excess reagents?
To find the limiting reagent, determine which reagent will give the smallest amount of
product.
40 slices of bread
Karen can only make 20 double cheeseburgers. The limiting reagent is the hamburger
patty. There are ten slices of bread and ten cheese slices in excess. Karen cannot
make more than 20 sandwiches because all the hamburger patties have been used up.
The excess reagent is N2. If you have 6.60 moles H2 then you will need
Therefore, the excess amount of N2 is 4.42 moles – 2.20 moles = 2.22 moles N2.
The theoretical yield is the maximum amount of product that would result if the limiting
reagent is completely consumed. It is the amount of product predicted by stoichiometry
(as shown in the above example).
The actual yield is the quantity of the desired product actually formed.
If in the example given above, only 54.0 g NH3 were produced, then the actual yield is
54.0 g; the theoretical yield is 78.0 g and the % yield is:
NAME: ________________________________________________________
GRADE & SECTION :_____________________________________________
ACTIVITY SHEETS
Activity 14
A. Silver metal reacts with sulfur to form silver sulfide according to the following
reaction: (8 points)
2Ag (s) + S(s) → Ag2S (s)
a. Identify the limiting reagent if 50.0 g Ag reacts with 10.0 g S.
b. What is the theoretical yield in g of Ag2S produced from the reaction?
c. What is the amount in g of the excess reactant expected to remain after the reaction?
d. When the reaction occurred, the amount of Ag2S obtained was 45.0 g. What is the
percent yield of the reaction?
B. Reflection: What do you think are your limitations? How do you cope with the
limited sources you have? (5 points)