Name Period Date Engage-Atoms 1. What does Bill cut in half?
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1 Name Period Date Engage-Atoms 1. What does Bill cut in half? 2. By cutting this item in half he tries to prove that there are pieces that are uncut- table called (which are too small to see even with a regular microscope). 3. Protons have a charge. 4. Neutrons have charge, they are neutral. 5. buzz (circulate) around outside the nucleus. 6. The flow of electrons from one atom to another is called. 7. Atoms are mostly space. 8. Atoms are so small; you can put 1,000,000 in the head of a. 9. are the basic building blocks of all matter. 10. Atoms are like and molecules are like in our universal alphabet. 11. All matter is made up of &. 12. Water (H 2O) is parts hydrogen and part oxygen. 13. A water molecule is like ears. 14. The number of in the nucleus makes one atom different from another. 15. The periodic table is arranged by or periods. 16. There are elements that occur naturally. Part One Atomic Theory Guided Notes 1 (slides 1-37) Notes Atomic Models 1. in (400 B.C.) stated that matter is made up of indivisible particles. He called these indivisible particles. 2. Around 1800 stated that all matter is made up of extremely small particles which he called. This was the real beginning of the modern atomic theory. 3. He stated that atoms of a given element are identical in,, and other properties.
2 4. Dalton s Atomic Theory is the basis of the, which states that a chemical compound contains the same element in the same ratio no matter the source or size of the sample, and the, which states that the same elements can combine in different proportions to form different compounds, and the which states that matter cannot be created nor destroyed. 5. Draw the Dalton model of the atom. 6. In 1897,, using the CRT (Cathode Ray Tube) for his experiment, discovered the. His model of the atom is known as the Plum-Pudding model. 7. Draw the Thomson model of the atom. 8. Next, the was discovered. 9. The that has no charge was discovered by J. Chadwick. 10. Later around 1911 performed the gold foil experiment and discovered that the atom is mostly empty space except for a small dense positive piece at the center. 11. He named this positively charged center of the atom the. 12. Draw the Rutherford model of the atom.
3 13. Around 1913, extended this theory of atomic structure. He stated that travel around the nucleus in orbits of certain energies. 14. In this model, he stated that in order to move from the original or state to an excited state, an electron must absorb an energy quantum and must an energy quantum to move back toward the nucleus to its original state. 15. Draw the Bohr model of the atom. Part II Subatomic Particles Guided Notes (slides 38-46) 1. The symbol for an electron is, the charge on the electron is, and the mass of an electron is. 2. The symbol for a proton is, the charge on the proton is, and the mass of a proton is. 3. The symbol for a neutron is, the charge on the neutron is, and the mass of a neutron is. 4. Atomic number is the in the nucleus. 5. determines the kind of atom. 6. In a neutral atom the number of is the same as the number of protons. 7. Mass number is plus. 8. The nuclear symbol of the element consists of the, the at the upper left and the at the lower left.
4 GENERIC EXAMPLE: 1. Find the number of protons number of neutrons number of electrons Mass Number 2. Find the number of protons number of neutrons number of electrons Mass Number 3. If an element has an atomic number of 34 and a mass number of 78 what is the - number of protons - number of neutrons - number of electrons - nuclear symbol 4. If an element has 91 protons and 140 neutrons what is the Mass number number of electrons nuclear symbol 5. If an element has 78 electrons and 117 neutrons what is the Mass number number of protons nuclear symbol
5 Part III Isotopes Guided Notes (slides 47-55) 1. are atoms of the same element with numbers of neutrons. 2. have different mass numbers 3. is the unit for atomic mass. 4. is 1/12 of the mass of a carbon-12 atom. Calculating Average Atomic Mass of Isotopes 1. To calculate the average atomic mass that is listed on the periodic table, Samples: the atomic mass of each isotope by it s percent abundance (expressed as a decimal), then the results. Calculate the atomic mass of copper if copper has two isotopes. 69.1% has a mass of amu and the rest has a mass of amu. Magnesium has three isotopes % magnesium 24 with a mass of amu, 10.00% magnesium 25 with a mass of amu, and the rest magnesium 25 with a mass of amu. What is the atomic mass of magnesium? Summary (slide 55): Atomic Number is the number of. Atomic Mass is the number of and. Isotopes have different numbers of.
6 Name Period Date Isotopes video: 1. To start off this lesson, we are comparing to to help you remember how to compare and contrast different isotopes of atoms. 2. Three different types of apples compared are the crab apple, the golden delicious apple and the. 3. The fictional mass given to the apples ( apple mass unit ) were 1, 2 & a.m.u. 4. The nucleus contains both & -- both of which are the primary contributors to the mass of the atom. 5. The mass of the is not significant enough to keep track of. 6. The number of protons an atom has will determine which type of it is. 7. The number of neutrons of an atom are where things get. 8. Isotopes have the same number of protons but different numbers of. 9. Hydrogen has isotopes. 10. Both protons and have a mass of about 1 amu (atomic mass unit). 11. The most common hydrogen isotope has one proton and zero neutrons, has a mass of 1 amu is called and make over 99.98% of all hydrogen atoms. 12. The next most common isotope of hydrogen is called deuterium and its nucleus contains 1 proton and 1 neutron giving it a mass of amu. It makes up less than 0.02% of the population of hydrogen atoms. 13. The last isotope is called and has 2 neutrons and 1 proton in its nucleus giving it a mass of 3 amu. Very little exists and it is very unstable. 14. If you were asked what is the mass of a hydrogen atom, you would need to know which of hydrogen.
Nuclear Chemistry. Atomic Structure Notes Start on Slide 20 from the second class lecture
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ATOMIC STRUCTURE. Name: Period: Date: 1) = a generalization of scientific observations that what happens (does explain)
ATOMIC STRUCTURE Name: Period: Date: I. LAW vs. THEORY: 1) = a generalization of scientific observations that what happens (does explain) 2) (model) = a set of assumptions used to explain observations