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For more information, please see full course syllabus of Physical Science
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Lecture Comments (9)

0 answers

Post by Christina Ho on September 21, 2014

What is the meaning of less energy elections or higher energy electrons in an atom? What is the difference of those atoms with different energy level ? Thanks .

2 answers

Last reply by: Carroll Fields
Wed May 28, 2014 10:24 AM

Post by jianhua Ling ling on December 3, 2013

Can you explain quarks more? I'm confused.

1 answer

Last reply by: Arvind Ganesh
Mon Mar 23, 2015 6:47 PM

Post by sushma penmetsa on February 14, 2013

how about having some quizzes based on the material?

0 answers

Post by Professor Ebs on January 31, 2013

That's a good question. We just pair them to see the electrons available for bonding. The electrons do not move together, just in similar spaces. Their similar negative charges and high amounts of energy prevent them from being too close to one another.

0 answers

Post by Erika Porter on January 31, 2013

In an atom do the electrons stay in groups or do they flow apart from one another?Do we just pair them so that we can see the non-paired electrons free for bonding?

0 answers

Post by Jona James on September 9, 2012

love your teaching style...#max pizzazz,, rock on :]

Atoms and Elements

  • An atom is the smallest particle of any element, which is a pure form of matter.
  • Atoms can be broken down into subatomic particles: protons, neutrons, and electrons
  • An atom is made up of an electron cloud around a nucleus
  • Electrons constantly moving around the nucleus make up the cloud, protons and neutrons clumped together make up the nucleus
  • Protons and neutrons are make up of smaller particles called quarks
  • In a neutral atom, the number of protons = the number of electrons = the number of neutrons.
  • Electrons in the electron cloud have different amounts of energy. The model of electron configuration places electrons in seven energy levels.
  • The electrons in energy levels closest to the nucleus have less energy than those electrons in levels further from the nucleus.
  • Electrons fill the energy levels from the inner levels to the outer levels.
  • Inner levels are completely filled with 8 electrons before electrons are placed in the next level out. The first level is filled at 2 electrons.
  • The atomic number gives the number of protons in one atom of the element.
  • ISOTOPES are atoms of the same element that have different numbers of neutrons.
  • Isotopes are named with the symbol and the mass number.

    MASS NUMBER is the sum of protons and neutrons in an atom.

Atoms and Elements

What are the three types of subatomic particles?
Protons, neutrons, and electrons
Where do you find the subatomic particles that make up an atom?
Protons and Neutrons make up the nucleus; Electrons are in constant motion around the nucleus.
What electric charges do the subatomic particles have?
Neutrons have no charge, protons are positive, electrons are negative.
What is the overall charge of an atom that has 3 protons, 3 neutrons, and 2 electrons?
The charge is +1.
The first electron level is filled with how many electrons?
2 electrons fill the inner level
What tells you the number of protons an atom has?
The atomic number of the element
How do you find the mass number of an atom with 3 protons, 3 neutrons, and 2 electrons?
Add the protons and neutrons the atom has a mass number of 6.
What is the mass number of the isotope named Li-5?
The mass number is 5.
The isotope Li-5 has how many neutrons? (Li = Lithium = atomic number=3)
2 neutrons mass number atomic number = number of neutrons)
What makes Nitrogen with an atomic number of 7 different from Oxygen that has an atomic number of 8? (What makes the atomic numbers different?)
Nitrogen atoms have 7 protons and Oxygen atoms have 8 protons.

*These practice questions are only helpful when you work on them offline on a piece of paper and then use the solution steps function to check your answer.


Atoms and Elements

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Atoms 0:05
    • Atoms
  • Atomic Structure 1:01
    • Electron Cloud
    • Nucleus, Protons, and Neutrons
    • Quarks
  • Protons, Neutrons, Electrons 2:40
    • Protons, Neutrons, Electrons: Location
    • Protons, Neutrons, Electrons: Electric Charge
    • Examples
  • Electron Configuration 5:32
    • Electron Configuration
  • Elements 12:22
    • Atomic Number
    • Carbon
    • Oxygen
    • Important Elements for Living Things
  • Isotopes 17:04
    • Isotopes
  • Example 1: Atomic Structure and Electrical Charge 21:16
  • Example 2: Electron Configuration 23:13
  • Example 3: Electron Configuration 24:57
  • Example 4: Use the Periodic Table to Complete the Table Below 26:08