Name: ______________________
LIFELINE WEEK 2 FOLLOW-ALONG SHEET
(CHEMISTRY BASICS)
**Reminder- Upload your personal profile picture to Moodle by
Friday, Jan. 17th at 11:59 PM**
 1/20/14- MLK DAY (Monday students must attend the Lifeline
session they signed up for)
Main topics:
 Hierarchy of Biological Order
 Matter and the Atom
 Elements
 Periodic Table
 Atomic Number and Mass Number
 Orbitals and Energy levels
 Compounds
List the Hierarchy of Biological Order:
1.
2. Molecules
3.
4.
5. Tissues
6.
7.
8.
Why Does it “Matter” Anyways?
The universe is made up mostly of _____________ and energy.
What are the two main characteristics of matter?
1.
2.
Can the air be classified as matter? ________
____________ = Pull of gravity on mass.
The Atom
The ____________ _________of matter that still retains the
properties of an element.
Subatomic Particles (Protons, Electrons, and Neutrons)
 ____________ are positively charged
Mass: 1 amu (atomic mass unit)
 ____________ are electrically neutral
Mass: 1 amu (atomic mass unit)
 ____________ are negatively charged
So small the mass is negligible *
 (Atoms have even smaller pieces like nucleons and
quarks…discovered by geeks with particle accelerators).
Protons and neutrons are located inside the _____________.
The nucleus is small, dense, and + charged.
Electrons move ______________________. They are found in
________________.
Elements
All forms of matter are composed of chemical elements.
An element is a substance that cannot be _________ _________ to
a simpler substance by chemical means.
Elements are made up of only _______ kind of atom.
Examples: ___________________________
Which 4 elements make up 96% of living matter?
1.
2.
3.
4.
The Periodic Table
Elements are arranged in order of increasing atomic number from:


All elements have their own symbol:
Carbon = _____
___________ = He
Oxygen = _____
What is the symbol for Sulfur? ______
What is the symbol for Potassium? ______
Which element is represented by Fe? by Ca?
Fe = _________
Ca = __________
Atomic Number
= The ________________ in the nucleus.
Carbon has _____ protons; oxygen has ____ protons.
The atomic number is __________ per element!
Unless otherwise stated, atoms are electrically neutral, so…
_________________ = # of electrons.
What is the atomic number of H? _____
What is the atomic number of Ne? _____
How many protons (+) are in Na? _____
How many protons (+) are in Zn? _____
How many electrons (-) are in Li? _____
How many electrons (-) are in Si? _____
What about Neutrons?
Mass Number = _______________ + ________________
Why is the mall of the electron(s) not included in the total mass
number? _______________________________________
Rearrange the equation: ________________ - ________________
Orbitals
 The 3-dimensional space where an electron is found 90% of the
time is called an _____________.
 No more than _____ electrons can occupy the same orbital.
Energy Levels
 The different states of potential energy that electrons have in an
atom are called ____________________ or
_____________________.
 Chemical behavior of an atom: Determined by the distribution
of electrons in the atom’s electron shells.
 Number of ______________ electrons determines
________________.
 The _________ shell is closest to the nucleus. Electrons in this
shell have the lowest energy (considered to be “stable”).
 Electrons in the _________ shell have more energy; electrons
in the third shell have more energy still, etc.
 As electrons are added, they tend to occupy the lowest
available shell.
 1st electron shell (N=1)
Contains the 1s ___________ only.
 1 orbital = holds a max. of 2 electrons
 (s orbital)
 2nd electron shell (N=2)
 Contains the 2S and 2P subshells
 Has _____ orbitals = holds a max. of 8 electrons (4
orbitals x 2 electrons each)
 (s, px, py, pz orbitals)
 REMEMBER: No more than 2 electrons can occupy the
same orbital!!!
Electron Configuration = the particular distribution of electrons
among the available orbitals within an atom.
Compound
 A substance consisting of two or more elements combined in a
_________ __________.
Ex :
H2O (water)
NaCl (sodium chloride = table salt)
C6H12O6 (glucose)
 In these compounds, what do the subscripts indicate?
If there is no number, there is only _______ atom present.
***All compounds are molecules, but not all molecules are
compounds.
Question #1) Where are the protons and neutrons located in an
atom?
Question #2) What is the maximum number of electrons that an
orbital may hold?
Question #3) Which 4 elements make up 96% of living matter?
Question #4) Mass number = _________ + _________
Question #5) What are the two main characteristics of matter?
Question #6) What element is represented by atomic number 16?
How many neutrons and electrons does it have?
Question #7) What element is represented by atomic number 18?
How many protons, electrons and neutrons does it have?
Question #8) Draw the fluorine atom using Bohr’s model. What
is the electron configuration for fluorine?
***Don’t forget to complete your homework!!!!***