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Homework: Review Notes Chapter 4 Packet

Homework: Review Notes Chapter 4 Packet. Chapter 4 Section 1. Introduction to Atoms. The Modern Atomic Model. In 1932, scientist James Chadwick discovered another particle in the nucleus of the atom Neutron Hard to detect due to no electric charge Nearly the same mass as a proton.

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Homework: Review Notes Chapter 4 Packet

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  1. Homework:Review NotesChapter 4 Packet

  2. Chapter 4 Section 1 Introduction to Atoms

  3. The Modern Atomic Model • In 1932, scientist James Chadwick discovered another particle in the nucleus of the atom • Neutron • Hard to detect due to no electric charge • Nearly the same mass as a proton

  4. The Modern Atomic Model

  5. Particle Charges • Protons are positively charged (p+) • Electrons are negatively charged (e-) • Neutrons have no charge (n)

  6. Particle Charges

  7. Comparing Particle Mass • Although electrons may balance protons charge-for-charge, they cannot compare when it comes to mass. • Approximately 2000 electrons equal 1 proton • A proton and a neutron are about the same mass • Protons and neutrons make up nearly all the mass of an atom.

  8. Comparing Particle Mass

  9. Atomic Number • Every atom of a given element has the same amount of protons • All forms of oxygen have the same number of protons (8) • All forms of carbon have the same number of protons (6) • The number of protons in a nucleus of an atom is the atomic number.

  10. Atomic Number

  11. Isotopes and Mass Number • Atoms of the same element that have a different number of neutrons are called isotopes. • An isotope is identified by its mass number, which is the sum of the protons and neutrons in the nucleus of the atom.

  12. Isotopes Assignment • You’re task is to diagram the three different carbon isotopes (pg. 130) • You will need to explain: • Why each carbon atom is considered an isotope? • How many protons and neutrons help compose each carbon isotope? • Which isotope of carbon has the largest mass number?

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