6.7 the structure of the atom
DESCRIPTION
6.7 The Structure of The Atom. ( p.234-240). Inside the Atom:. atom. The _____ is the smallest particle of an element that has the same properties of the element. Atoms do not have a CHARGE . The atom is composed of many smaller ___________ particles. - PowerPoint PPT PresentationTRANSCRIPT
6.7 THE STRUCTURE OF
THE ATOM(p.234-240)
INSIDE THE ATOM:
• The _____ is the smallest particle of an element that has the same properties of the element. • Atoms do not have a CHARGE.• The atom is composed of many smaller ___________ particles. • 3 Main Types of Subatomic Particles: __________ and __________, which make up the ________ and ___________, which move in specific regions around the nucleus.
atom
subatomic
protonsneutrons nucleus electrons
TERMINOLOGY
• ________________: The number of protons in the nucleus of an atom. This identifies an atom as a particular element (the # of protons never changes).
• ______________: the ________ mass of the _________ occurring isotopes of an element.• The sum of the number of protons & neutrons in an atom.• Protons and neutrons contribute nearly all the mass
of an atom.
Atomic Number
Atomic Mass naturallyaverage
ATOMIC MASS
•Atomic Mass refers to the “weight” of the atom.• It is derived at by adding the number of protons with the number of neutrons.
HThis is a helium atom. Its atomic mass is 4 (protons plus neutrons).
What is its atomic number?
TERMINOLOGY
• _______________________: the number of rings around the nucleus that contain the electrons. (Period Number).
• _____________: The electrons in the outermost shell (Group Number)
• ___________: The outermost shell
Valence Electron
Valence Shell
Orbits / Shells / Energy Levels
Subatomic Particle
Charge Location Relative Mass
Protons
Neutrons
Electrons
+’ve Nucleus 1 AMU
Neutral Nucleus 1 AMU
-‘ve Orbitals /
shells 1/2000* *
ATOMIC MASS UNIT (AMU)
•The unit of measurement for an atom is an AMU. It stands for atomic mass unit.•One AMU is equal to the mass of one proton.
ATOMIC MASS UNIT (AMU)
• There are 6 X 1023 or 600,000,000,000,000,000,000,000 AMU’s in one gram.• Remember that electrons are 2000 times smaller than one AMU.
Key TermsTry to find the following on the image…
• Nucleus• Protons• Neutrons
• Electrons• Orbits / shells /
energy levels• Valence Shell• Valence Electron
12
4
3
Energy LevelsValence
Electrons
Valence Shell
Lets See
What You
Know
Fill in the diagram on the following page… you MUST know all of these
terms….
REPRESENTING ELEMENTS:• The symbols that are used to represent the elements are the same throughout the world – the system is international.
• A common notation that scientists use to represent atoms of elements is called the _______________ ____________ ______________, which includes the _______ ___________ and ________ _____________ of an atom of an element.
StandardAtomic Notation Atomic
Number Atomic Mass
Review…. # of… in an ATOM of Carbon
Protons =
Neutrons =
Electrons =
Overall Charge =
# of Shells =
# of Valence Electrons =
? 3
? 4
? 2
? 5
? 1
REPRESENTING ATOMS:
•The Bohr-Rutherford model is a convenient way of representing the atomic structure of an element.•How to draw a Bohr-Rutherford Diagram: PAGE 236
EXAMPLES – FROM CLASS NOTE
• Potassium (K) 2-8-8-1 Sodium (Na) 2-8-1Hydrogen (H) 1 Oxygen (O) 2-6 • Carbon (C) 2-4 Silicon (Si) 2-8-4 Magnesium (Mg) 2-8-2 Aluminum (Al)
2-8-3 • Chlorine (Cl) 2-8-7 Argon (Ar) 2-8-8 Boron (B) 2-3 Calcium (Ca) 2-
8-8-2
• Lithium (Li) 2-1 Sulfur (S) 2-8-6 Neon (Ne) 2-8
LEWIS DOT DIAGRAM
• Simply show the number of valence electrons. • No reference to
number of shells/orbits/energy levels
HW QUESTIONS
•Pg 240
•Q 1-8