Transcript of atoms in an isotope

MODULE 1
CHAPTER 2
LECTURE OUTLINE
Types of Matter
(Chapter 1 Review):
• ATOM - The smallest particle of an element that retains the
chemical properties of that element.
• COMPOUND - Matter that is composed of 2 or more elements
combined in definite proportions.
• ELEMENT - Matter that is composed of only one type of atom.
• MOLECULE - A definite group of atoms that are chemically
bonded, i.e. tightly connected by attractive forces.
• MATTER - Anything that has mass and occupies space.
• SUBSTANCE - Matter that can not be separated by physical
techniques, and that has a unique set of properties.
Fundamental Building Blocks
• All matter is composed of 12 fundamental
building blocks
– 6 are called quarks and
– 6 are called leptons.
QUARKS
• QUARKS - composite particles that protons,
neutrons and other subatomic particles are made
from. There are 6 different types of quarks:
– Up & down,
– Charm & strange, and
– Top & bottom.
LEPTONS
• LEPTONS – are independent particles of 6
different types:
– Electrons & electron neutrino,
– Muon & muon neutrino, and
– Tau & tau neutrino.
PROTONS
• PROTONS – are defined as:
– positively charged subatomic particles with a charge
of +1.602x10-19 coulombs
– found inside the nucleus
– composed of 2 up quarks and 1down quark
– mass = 1.672622x10-24 g or 1.007276 AMU
* The elements atomic number ( Z#) = # protons
NEUTRON
• NEUTRONS – are defined as
–
–
–
–
electrically neutral subatomic particle
found inside the nucleus
composed of 2 down quarks and 1 up quark
mass = 1.674927x10-24 g or 1.008665 AMU.
NUCLEUS
• NUCLEUS – is defined as:
–
–
–
–
–
–
core of the atom
centrally located
positively charged
contains most of the atom's mass
very dense
small relative to the overall size of the atom
ELECTRONS
• ELECTRONS – are defined as:
– negatively charged subatomic particle with a charge of
-1.602x10-19 coulombs
– leptons
– found outside of the core of the atom
– mass = 9.1x10-28 g or 0.00055 AMU
– travel in orbitals around the nucleus
– mostly empty space
– occupies most of the size of the atom
ATOMS
• ATOMS – are defined as:
– smallest particle of an element that retains the
chemical properties of that element
– composed of the nucleus (core) surrounded by
electrons
ISOTOPES
• ISOTOPES – are defined as:
– Atoms of the same atomic number but different mass
B-10 = Boron has 10 mass units, 5 protons & 5 neutrons
B-11 = Boron also can have 11 mass units, 5p & 6n
Percent Abundance = # of atoms in an isotope x 100%
total # of all isotopes of that element
ATOMIC WEIGHT
• ATOMIC WEIGHT or ATOMIC MASS – are
defined as:
– Average mass of all naturally occurring isotopes of
that element
– See Table 2.2 on page 57
– Review Exercise 2.4 – Calculating Atomic Wt., pg. 58
– Review Screen 2.12 on the CD-ROM
CONCEPT OF A MOLE
MOLE – amount of substance that contains as
many elementary particles as there are atoms in
exactly 12 grams of the carbon-12 isotope
1 mole = 6.022 x 10 23 particles
- Just like 1 dozen eggs = 12 eggs
- 1 mole eggs = 6.022 x 10 23 eggs
MOLAR MASS
• MOLAR MASS – the mass in grams of one mole
of atoms of any element which is 6.022 x 10 23
atoms of that element
Ex. 1 mole of Na = 22.9898 grams of Na
1 mole of Na = 6.022 x 10 23 atoms of Na
22.9898g of Na = 6.022 x 10 23 atoms of Na
Conversion of Units
• Review Example 2.4 - Mass, Moles, and Atoms
pg. 60-61
• Review Example 2.5 - Mole Calculations pg. 61
** Use unit label to perform all conversions!
The Periodic Table
• View Screens 2.13 & 2.14 on the CD-ROM
• Go into the Interactive Periodic Table on the CDROM and familiarize yourself with its features.
• Read pages 62 – 72 in the text and pay particular
attention to the display on page 63.