1. Chapter 2: Introductory Chemistry
ANATOMY & PHYSIOLOGY
Chapter 2: Introductory Chemistry

2. Concepts of Matter matter - anything that occupies space and has mass
- may be changed both physically and chemically
physical change
- does not alter nature of substance
i.e.) change in state - ice to water
chemical change
- does change composition of substance
i.e.) fermentation of grapes

3. Concepts of Matter states of matter Gas no definite shape; no definite
volume. i.e.) air
Liquid
definite volume; conforms to
shape of container i.e.) blood;
interstitial fluid
Solid –
definite shape and volume i.e.) bones
d. Plasma

4. Chemical Reactions energy mass-less; does not take up space
measured by its effect on matter
ability to do work or to put matter into motion

5. Chemical Reactions Energy All forms of energy (4) exhibit both:
kinetic energy
when energy is moving objects; actually doing work - causing an effect
potential energy
inactive or stored energy

6. Concepts of Energy 4 forms of energy chemical energy
energy stored in the bonds of chemical substances and released when bonds are broken
electrical energy
energy resulting from movement of charged particles

7. Concepts of Energy 4 forms of energy radiant energy
energy that travels in waves; energy of the electromagnetic spectrum
mechanical energy
directly involved in putting matter into motion

8. Concepts of Energy energy form conversion
energy is easily converted from one form to another
energy conversions are inefficient;
some of the initial energy supply is lost (unusable) to the environment as heat

9. ?Question? Is it really lost? If not, where is it?
The statement has been made that “some energy is lost in every energy transformation.” Explain the meaning of this statement.
Is it really lost?
If not, where is it?

10. Intro to Chemistry Chemical Elements and atoms elements
unique substance that cannot be decomposed or broken down into simpler substances by ordinary chemical methods
118 (120) discovered elements; 92 occur naturally; 26 (28) produced artificially
4 different elements make up most of the body

11. Chemical Elements and atoms
four most abundant (making up
96 % of body’s mass) these elements are O,C,H & N
elements that make up approx.
3.8 % include Ca, P, K, S, Na, Cl, Mg, Fe
trace elements - additional 14 elements present in tiny amounts make up the balance of approx. 0.2% -include:
Al, B, Cr, Co, Cu, F, I, Mn, Mo, Se, Si, Sn, V, Zn

12. Chemical Elements and atoms
building block of an element
smallest particle that still retains its specific properties
two basic parts: nucleus and one or more electrons

13. Chemical Elements and atoms
an atom is a cluster of smaller (subatomic) particles and can be split into these
an atom loses the unique properties of its elements when it is split in its subparticles

14. Atomic Structure subatomic particles
three basic particles differing in their:
mass,
electrical charge, and
location within the atom
the electrical charge of a particle is a measure of its ability to attract or repel other charged particles

15. subatomic particles proton – positive charge neutron– neutral charge
electron – negative charge

16. subatomic particles
all atoms are electrically neutral; the number of protons must be balanced by the number of its electrons
protons and neutrons are clustered at the nucleus

17. subatomic particles
electrons orbit around the nucleus, forming a negatively charged electron cloud
most of the volume of an atom is empty space, and nearly all of the mass is concentrated in the nucleus

18. Differentiating elements/atoms
to identify a particular element:
atomic number
equal to the number of protons its atom contains
mass number
the sum of the protons and neutrons in its nucleus

19. Differentiating elements/atoms
atoms of different elements are composed of different numbers of subatomic particles
again, number of protons and electrons are equal; number of neutrons vary
light atoms tend to have equal number of protons, electrons, and neutrons
larger atoms have more neutrons than protons and electrons

20. Differentiating elements/atoms
isotopes
atoms of almost all elements exhibit two or more structural variations called isotopes
isotopes have the same number of protons and electrons, but vary in the number of neutrons they contain - thus,
has the same atomic number (same chemical properties) of the element, but has a different atomic mass
an element’s lightest isotope is more abundant than its heavier forms

21. Differentiating elements/atoms
radioisotopes
heavier isotopes of certain elements are unstable and decompose to become more stable
radioactivity – spontaneous atomic decay that involves:
ejection of particles
alpha (least penetrating)
beta
electromagnetic energy
gamma rays (most penetrating)

22. ?Questions?
Why is a study of basic chemistry essential to understanding human
physiology?
Matter and your body – how are they interrelated?
Matter occupies space and has mass. Describe how energy must be described in terms of these two factors.

23. ?Questions?
The statement has been made that “some energy is lost in every energy transformation.” Explain the meaning of this statement. (Direct your response to answering the question: Is it really lost? If not, where is it?)
According to Greek history, a Greek scientist went running through the streets announcing that he had transformed lead into gold. Both lead and gold are elements. On the basis of what you know about the nature of elements, explain why his rejoicing was short-lived.

24. ?Questions?
What four elements make up the bulk of all living matter? (Give both their names and their atomic symbols.) Which of these is found
primarily in proteins and nucleic acids?
List six other elements found in the body and
describe one way in which each is important to body functioning.
What is the relationship of an atom to an element?

25. ?Questions? All atoms are neutral. Explain the basis of this fact.
Complete this statement:
Chemical behavior results from
interactions of the ___________
found in the _______________ of the
atom.

26. ??Questions?? Define isotope.
If an element has three isotopes, which of them (the lightest, the one with an intermediate mass, or the heaviest) is most likely to be a radioisotope?
Why?
Define radioactivity.