BIOL 1081 Lecture Notes - Lecture 2: Atomic Number, Hydrogen Bond, Covalent Bond

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25 May 2018
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Learning Outcomes
Atoms, Elements, & Chemical Bonds Reading: Sections 2.1-2.3 in textbook and videos
1. Define element, compound, atomic number, atomic mass, and isotope.
Element-any substance that cannot be broken down to any other substance by
ordinary means
Compound-substance consisting of atoms of two or more elements that are
chemically bonded together
Atomic #-number of protons
Atomic Mass-sum of masses of protons and neutrons
Isotope-two or more atoms that have the same atomic number but a different
number of neutrons
2. Describe atomic structure, the characteristics of subatomic particles, and how they
determine chemical properties.
Atomic structure-A nucleus consisting of protons and neutrons. Electrons
surround nucleus
Protons- in nucleus, positive charge, equals atomic number
Neutrons- in nucleus, no charge, equals atomic mass
Electrons- surrounding, negative charge
Determine chemical properties because the number of electrons in an orbital.
---allows for reactivity
3. Give examples how isotopes can be used in biological research and medicine.
They are used for their radioactive properties to act as tracers in the body for
diagnostic and treatment purposes.
4. Explain the discrete energy levels in which electrons orbit the nucleus of an atom and
how this is related to potential energy.
K level- single orbital, 1s2 electrons
L level- 4 orbitals, 2s, 3 2p8 electrons
M level
o When completely filled, they are unreactive. When not filled, they look
to be filled, so they are considered reactive
5. Relate position in the periodic table to atomic structure and the formation of ions.
Period-principle energy level
Group- relating to the extent of subshells are filled
Elements with the same number of valence electrons are kept together in
groupsHalogens, Noble gases
Horizontal rows= by order of increasing atomic number
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