some basic concepts related to chemistry.

1. BASIC CONCEPT OF
CHEMISTRY
KEHKASHAN SABIR
(LECTURER)
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2. What is chemistry?
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3. Chemistry is a science that focuses on the composition
and properties between a variety of substances and
different forms of matter and their interaction with each
other.
Chemistry is also a physical science that analyzes various
atoms, molecules, crystals, and other aggregates of
matter.
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4. BIOCHEMISTRY
• Biochemistry or biological chemistry, is the study of chemical
processes within and relating to living organisms.
BIOLOGY CHEMISTRY
BIOCHEMISTRY
+
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5. WHAT IS NURSING ?
• On the other hand, nursing is an art and science.
• It interplays with other disciplines outside nursing such as social,
behavioral, and physical sciences.
• Nursing, as a profession is unique because it is focused on health
promotion, health maintenance, and health problems of
individuals and families.
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6. IMPORTANCE OF CHEMISTRY IN NURSING
1) Chemistry is important in nursing because it helps in
administering medicine to patients.
 Nurses must understand how particular
medicines will react in different patients.
 This helps to avoid wrong combinations
of drugs that can lead to adverse effects.
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7. 2) Chemistry will also guide the nurse understand the present condition of
the patient.
 Understanding the importance of
Sodium (Na), Potassium (K), Chloride
(Cl), Bicarbonate (HCO3), Carbon
dioxide (CO2), Oxygen (O), and other
electrolytes in the body will guide the
nurse to identify if his/her patient is
experiencing electrolyte imbalance.
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8. MORE APPLICATIONS OF CHEMISTRY IN NURSING?
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9. BASIC TERMS USED IN CHEMISTRY
• MATTER
• ATOM
• ELEMENT
• MIXTURE
• COMPOUND
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10. MATTER
• There are many possible definitions of matter. In science, the
matter is the term for any type of material.
• The matter is anything that has mass and takes up space.
• At a minimum, the matter requires at least one subatomic particle,
although most matter consists of atoms.
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11. Examples of Matter
Matter can include any of the following (and more, of course):
•Proton
•Atoms (e.g., a helium atom)
•Molecules (e.g., water, sugar)
•Compounds (e.g., table salt, silicon dioxide)
•Cat
•Tree
•House
•Computer
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13. ATOM
How many atoms are there in water?
The smallest unit of matter that has the
characteristic properties of a chemical element.
As such, the atom is the basic building block of
chemistry.
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14. STRUCTURE OF AN ATOM
• Like everything else, atoms have a few different things floating
around inside of them. These subatomic particles include:
• neutrons - with no charge
• protons - positively charged
• electrons - negatively charged
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15. • The protons and neutrons are in the atomic nucleus of the atom,
while the electrons orbit the atomic nucleus.
• Think of this as similar to the way the planets all orbit the sun.
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16. ELEMENT
• An atom is the part of an element.
• A particular element is composed of only one type of atom.
• Elements can combine with each other to form molecules via
chemical reactions.
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18. MOLECULES
• Molecules are what you get when those atoms
are combined.
• Unlike elements, molecules can be made from
the same or different elements.
• The key to a molecule is that two or more
atoms are bonded together.
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19. FOR EXAMPLE
• Water is a molecule made of hydrogen and oxygen.
• It’s actually made of two hydrogen atoms and one oxygen atom.
• You can also have molecules of a single atom bonded together like
two oxygen atoms.
• This makes up the oxygen humans breathe.
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20. MIXTURE
• Mixtures are substances that are formed by physically mixing two
or more substances.
• Mixtures are mainly of two types i.e. homogenous mixtures and
heterogeneous mixtures.
DIFFERENTIATE BETWEEN HOMOGENOUS AND HETEROGENEOUS
MIXTURES WITH EXAMPLES.
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21. COMPOUNDS
• Compounds are substances that can be formed by chemically
combining two or more elements.
• Compounds can be of three types, which are: covalent
compounds, metallic compounds, and ionic compounds.
Note: Compounds can be classified as organic compounds or inorganic
compounds depending on the presence of carbon in the molecular structure.
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23. WHAT IS BLOOD ??
• IS BLOOD A MIXTURE OR COMPOUND??
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24. CHEMICAL FORMULA
• A chemical formula tells us the number of atoms of each element
in a compound.
• It contains the symbols of the atoms of the elements present in the
compound as well as how many there are for each element in the
form of subscripts
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26. MOLECULAR FORMULA
• The molecular formula, sometimes known as the true formula, tells
us the actual number of the different elements in one molecule of
a compound.
• In a molecular formula, each element is written as its symbols in
the periodic table, and the number of atoms for each element is
shown by the subscript (the small number to the lower right of the
element).
• Here are some examples of molecular formulas:
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28. EMPIRICAL FORMULA
• Empirical formula is defined as the simplest ratio of whole
numbers of elements that make up a compound, and this type of
formula is derived from experimental data.
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30. STRUCTURAL FORMULA
• When we simply write the molecular formula, we do not know how
the atoms are arranged or which atoms are bonded to each other.
• The structural formula shows both the actual number of atoms of
elements in a compound, how the atoms are arranged and which
atoms are bonded to one another.
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32. ACTIVITY
• Write molecular formula, empirical formula and structural formula
of:
1) Water
2) Carbon dioxide
3) Methane
4) Glucose
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33. SOLUTION
Molecular formula Empirical formula Structural formula
H20 H20
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34. Molecular Formula Empirical Formula Structural Formula
CO2 CO2
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35. Molecular Formula Empirical Formula Structural Formula
CH4 CH4
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36. Molecular formula Empirical formula Structural formula
C₆H₁₂O₆ CH2O
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37. CHEMICAL REACTIONS
• A chemical reaction is in which the bonds are broken within
reactant molecules, and new bonds are formed within product
molecules in order to form a new substance.
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38. BASIC CONCEPTS OF CHEMICAL REACTIONS
• A Chemical Reaction is a process that occurs when two or more
molecules interact to form a new product(s).
• Compounds that interact to produce new compounds are called
reactants whereas the newly formed compounds are called products.
• Chemical reactions play an integral role in different industries, customs
and even in our daily life. They are continuously happening in our
general surroundings; for example, rusting of iron, pottery,
fermentation of wine and so on.
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39.  In a chemical reaction, a chemical change must occur which is
generally observed with physical changes like precipitation,
heat production, color change, etc.
 A reaction can take place between two atoms or ions or
molecules, and they form a new bond and no atom is destroyed
or created but a new product is formed from reactants.
 The rate of reaction depends on and is affected by factors like
pressure, temperature, the concentration of reactants.
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41. 1. SYNTHESIS REACTIONS
Two or more reactants combine to make 1 new product.
Examples:
C(s) + O2(g) → CO2(g)
H2O(l) + SO3(g) → H2SO4(aq)
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42. 2. DECOMPOSITION REACTIONS
A single reactant breaks down to form 2 or more products.
Examples:
H2CO3(aq) → H2O(l) + CO2(g)
CaCO3(s) → CaO(s) + CO2(g)
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43. 3. SINGLE-REPLACEMENT REACTIONS
A single element replaces a similar element of an adjacent reactant
compound.
Examples:
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
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44. 4. DOUBLE-REPLACEMENT REACTIONS
Two ionic compounds exchange ions, producing 2 new ionic
compounds.
Examples:
NaCl(aq) AgNO3(aq) → NaNO3(aq) + AgCl(s)
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
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45. 5. COMBUSTION REACTIONS
A single element or compound combines with oxygen gas releasing
energy. This rapid oxidation is called burning.
Examples:
C(s) + O2(g) → CO2(g) + energy
2Mg(s) + O2(g) → 2MgO(s) + energy
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46. CHEMICAL EQUATION
• Chemical equations are symbolic representations of chemical
reactions in which the reactants and the products are expressed in
terms of their respective chemical formulae.
• Chemical reactions can be represented on paper with the help of
chemical equations, an example for which is represented below
(for the reaction between hydrogen gas and oxygen gas to form
water).
2H2 + O2 → 2H2O
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47. It can also be observed that there are coefficients assigned to each of
the symbols of the corresponding reactants and products.
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49. Regardless of the absolute numbers of molecules involved, the ratios between the
numbers of molecules of each species that react (the reactants) and molecules of
species that form (the products) are the same and are given by the chemical
equation.
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50. IONIC CHEMICAL EQUATIONS
• In ionic chemical equations, the electrolytes (substances that
dissociate into ions when dissolved in polar solvents) are split up
and written as separate ions.
Chemical Equation: CaCl2 + 2AgNO3 → Ca(NO3)2 + 2AgCl↓
Ionic Equation: Ca2+ + 2Cl– + 2Ag+ + 2NO3– → Ca2+ + 2NO3– +
2AgCl↓
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51. THANK YOU
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