3. Chemistry
• Chemistry can be defined as the study of the composition,
structure, and properties of material substances and the
changes associated with these substances.
4. Importance of chemistry in
nursing
• Chemistry gives nurses the knowledge about compounds
like medicine.
• It teaches them what medications are made of and what they
will do to the patient when it is administered.
• Understanding chemistry will allow nurses to know why
medications within the same classification or similar names do
not work the same.
5. Atom
• The smallest particle of a chemical element that can exist.
• The atom is the basic particle of the chemical elements, and the
chemical elements are distinguished from each other by the
number of protons that are in their atoms
• An atom is a particle that consists of;
• Nucleus of protons and neutrons
• Electrons surrounds the nucleus .
6. Element
• Elements is a species of atoms that have the same number of
protons in their atomic nuclei.
• Although an element’s atoms have the same number of
protons, they can have different numbers of neutrons and
hence different masses.
7. Types of Elements
• The elements are arranged in the periodic table and are split
depending upon their groups as either metallic or non-metallic.
• Metallic is further classified into Main Group Metals,
Transition Metals, and f-block metals. These are again further
divided, depending upon their properties.
11. Types of compound
• Compounds can be classified into two types, molecular
compounds and salts.
• In molecular compounds, the atom binds each other through
covalent bonds.
• In salts, it is held together with ionic bonds.
14. Example
•Air: a mixture of various gases like
oxygen, carbon dioxide, nitrogen,
argon, neon, etc.
• Ink: A mixture of coloured dyes.
Gunpowder: A mixture of sulfur,
potassium nitrate and carbon.
15. Structure of atom
•atom, smallest unit into which matter
can be divided without the release of
electrically charged particles. It also is
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.
16. Atom consist of
• Most of the atom is empty space. The rest
consists of a positively charged nucleus
of protons and neutrons surrounded by a
cloud of negatively charged electrons. The
nucleus is small and dense compared with
the electrons, which are the lightest
charged particles in nature.
• Electrons are attracted to any
positive charge by their electric force; in an
atom, electric forces bind the electrons to
17. Atomic number
• The single most important characteristic of an atom is its
atomic number (usually denoted by the letter Z), which is
defined as the number of units of positive charge
(protons) in the nucleus.
• For example, if an atom has a Z of 6, it is carbon, while
a Z of 92 corresponds to uranium. A neutral atom has an
equal number of protons and electrons so that the positive
and negative charges exactly balance.
• Since it is the electrons that determine how one atom
interacts with another, in the end it is the number of
protons in the nucleus that determines the chemical
properties of an atom.
18. Atomic mass
• The number of neutrons in a nucleus affects the mass of
the atom but not its chemical properties. Thus, a nucleus
with six protons and six neutrons will have the same
chemical properties as a nucleus with six protons and
eight neutrons, although the two masses will be different.
•
• Nuclei with the same number of protons but different
numbers of neutrons are said to be isotopes of each other.
All chemical elements have many isotopes.
19. Orbits or energy level
• Nucleus of an atom is surrounded by the
orbits or shell
• Electron continuously revolve in the shell
• Energy in the shell is inversely proportional
to the distance between nucleus and shell.
20.
21. Properties of periodic table
•Group;
•The vertical columns on the periodic
table are called groups.
•All the members of a family of
elements have the same number of
valence electrons and similar
chemical properties.
22. Periods
• The horizontal rows on the periodic table
are called periods.
• Number of shell increases with increase in
periods.
• There are 8 periods in periodic table
23. Electron affinity
•The energy released when an electron
is added to a gaseous atom which is in
its ground state to form a gaseous
negative ion is defined as the first
electron affinity.
24. Ionization energy
• The ionization energy, EI, of an atom/ion is
the minimum energy which is required to
remove an electron of an atom.
• The unit of ionization energy is kJ/mol.
26. 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.
27. Importance of Chemical Formula
• Chemical formulae provide insight into the
chemical composition of a compound.
• They also represent the ratios in which the
constituent elements combine to form the
compound.
• The chemical formula of a compound is crucial
while representing it in a chemical equation.
• Chemical formulae can also be employed to
represent ions, free radicals and other chemical
species.
28. Types of Chemical Formula
• 1. Molecular Formula:
• The molecular formula provides insight into the
number of elements present in a compound. In
molecular formulae, the elements are denoted by
their respective symbols (as in the periodic table)
and the number of atoms of each element in the
molecule is written in subscript.
• For example- the molecular formula for glucose
is C6H12O6.
29. • 2. Empirical Formula:
• The empirical formula of a chemical compound
represents the ratio of the elements present in that
compound. Empirical formulae are usually
obtained based on the analysis of experimental
data. The empirical formula for glucose is CH2O.
Empirical Formulae can be derived from the
molecular formulae.
30. • 3. Structural Formula:
• As the name suggests, the structural
formula of a chemical compound provides
insight into the arrangement of the atoms
in the molecule.
31. Chemical reactions
•Chemical reactions occur when
chemical bonds between atoms are
formed or broken.
•Bond may be ionic or covalent.
• The substances that go into a
chemical reaction are called the
reactants, and the substances produced
at the end of the reaction are known as
the products.
32. Equations
• Equations are the representation of the chemical reaction
by using the formulas
• The left-hand side of a chemical equation represents the
reactants and the right-hand side represents the products.
33. Bonding
• Bond formed when;
• Electrons transferred from one atom to
another.
• Electrons shared between neighboring
atoms.
• There are two types of the bond
• 1. ionic
• 2. covalent
• .
34. Ionic bond
•Formed when atom loss or gain
the electrons
•such as
•NaCl: sodium chloride.
• NaF: sodium fluoride.
35. Covalent bond
• Formed by the mutual sharing of electrons
• It may;
1. single covalent bond
• Sharing of 1 pair
2. double covalent bond
• Sharing of 2 pair
3. triple covalent bond
Sharing of 3 pair
water (H₂O), and methane(CH₄).
36. Redox reaction
• Oxidation–reduction reactions, commonly
known as redox reactions, are reactions
that involve the transfer of electrons
from one species to another.
• The species that loses electrons is said to
be oxidized, while the species that gains
electrons is said to be reduced.
37. Acid & Base
Arrhenius definition;
• Arrhenius first defined acids as compounds
which ionize to produce hydrogen ions, and bases
as compounds which ionize to produce hydroxide
ions.
Lowry-Bronsted
• According to the Lowry-Bronsted definition, an
acid is a proton donor and a base is a proton
acceptor.
38. Lewis definition
• According to the Lewis definition,
• acids are molecules or ions capable of
coordinating with unshared electron pairs, and
bases are molecules or ions having unshared
electron pairs available for sharing with acids.
• To be acidic in the Lewis sense, a molecule must
be electron deficient. This is the most general
acid base concept.
39. pH definition
• A figure expressing the acidity or alkalinity
of a solution on a logarithmic scale on
which 7 is neutral, lower values are more
acid and higher values more alkaline.
• The pH is equal to −log10 c, where c is the
hydrogen ion concentration
in moles per litre.
40. Salt
• Any chemical compound formed from the
reaction of an acid with a base, with all or part of
the hydrogen of the acid replaced by a metal.
41. Assignments
• 1. learn properties of periodic table
• Practice covalent and ionic bond, equations, chemical
formulas,.
• Learn concept of acid and base by different scientist
