Atom overview and subatomic particles

1.

ATOM OVERVIEW
and
SUBATOMIC
PARTICLES
• Elements are made up of atoms.
• Atoms are made up of protons and
neutrons located within the nucleus, with
electrons in orbitals surrounding the
nucleus.

DEFINITIONS
• Proton: positively charged particle in
the nucleus of all atoms
• Neutron: uncharged subatomic
particle in the nucleus
• Electron: negatively charged
subatomic particle that occupies
orbitals around the atomic nucleus
• Nucleus: core of atoms, occupied by
neutrons and protons
• Atomic number: number of protons in
the atomic nucleus, determines the
element
• Atomic Mass: total number of protons
and neutrons in the nucleus of an
element’s atom
• Isotope: element that differ in the
number of neutrons
• Radioisotope: isotope with instable
nucleus

3.

Characteristics
of Subatomic
Particles
• Electrons have a negative charge and no mass.
• Protons have a positive charge and a mass of 1 unit.
• Neutrons have no electrical charge and a mass of 1 unit.

4.

JUST FEW OF THEM ARE
ESSENTIAL TO LIFE, DIVIDED INTO:
Periodic
table of
Elements
• BULK ELEMENTS: C, O, H, N
(Carbon, Oxygen, Hydrogen, Nitrogen)
• TRACE ELEMENTS: Fe, K, Na, Zn,
Ca (Iron, Potassium, Sodium, Zinc,
Calcium)
Trace elements (or trace metals)
are minerals present in living tissues in
small amounts

5.

1. The abundance of elements in different
living organisms is in a given concentration
range;
Trace
elements
2. The decreasing of abundance of
elements causes physiological changes
(diseases);
3. Administration of missing trace elements
improve the physiological condition.
They take part in the metabolism.
4. The elements have defined biochemical
functions.

6.

1. Transport of biological small molecules
pl. O2-transport: hemoglobin (Fe), hemocianin (Cu)
O2-storage: mioglobin (Fe)
Roles of
trace
elements
2. Activation of molecules: metalloenzymes, enzymes activated
by metal ions:
a) catalysing of redox processes (Fe, Cu, Mn, Co, Mo, Ni)
biological oxidation, reduction of substrate
b) catalysing of acid-base processes (Zn)
3. Seconder conformation of macromolecules
– determination of conformation of enzymes
– determination of conformation of proteins, nucleic acids
4. Metabolism of microelements
– uptaking, transport, storage of trace elements

7.

Chemical bond: an attractive force that arises
between two atoms when their electrons interact.
Covalent bond: chemical bond in which two atoms
share a pair of electrons.
Hydrogen bond: attraction between a bonded
hydrogen atom and another.
DEFINITIONS
Ionic bond: bond in which a strong mutual attraction
forms between ions of opposite charge.
Molecule: group of two or more atoms joined by
chemical bonds
Compound: type of molecule that has atoms of more
than one elements
Polarity: Any separation of charge into distinct
positive and negative regions.

8.

What is a Chemical
bond?
Atoms accept, share, and donate
electrons; Whether an atom will
interact with other atoms depends
on how many electrons it has. A
chemical bond is the union of the
electron structures of atoms.
Atoms with an unfilled outer shell
tend to interact with other atoms in
ways that fill the shell, such as
forming chemical bonds.
Atoms with a filled outer shell are
inert- they do not form bonds.

9.

Valence electron
• Valence electron is an electron that is
associated with an atom, and that can participate
in the formation of a chemical bond; occupies
outermost shell.
https://www.youtube.com/watch?v=4OKy782ePKM

10.

Types of
bonds:
Three types of bonds:
1. IONIC (giving up of e-); STRONG
2. COVALENT (non- polar and polar)
sharing of e-; STRONG
3. HYDROGEN between (hydrogen atom
which usually has a partial + charge, is
attracted to an atom w/ a partial - charge)
WEAK

Atom overview and subatomic particles

1.

2.

3.

4.

5.

6.

7.

8.

9.

10.

11.

12.

13.

14.

15.