Number of Protons, netrons, and electrons.pptx

Grade 8 Periodic Table

1. Tuesday, February 2, 20XX Sample Footer Text 1 INTRODUCTORY ACTIVITY

2. Number of Protons, netrons , and electrons in a particular atom Prepared by: Cristy R. Villamor- Gesta

3. Objectives Identify the relationships of number of protons, electrons, and neutrons in atom Calculate the number of electrons, protons and neutrons in an atom Show determination in getting the number of electrons, protons, and neutron Show interest in interpreting shorthand notations for isotopes and atoms. Tuesday, February 2, 20XX Sample Footer Text 3

4. Tuesday, February 2, 20XX Sample Footer Text 4 The atomic number of an element is determined by the number of protons in it, and it is used to differentiate one element from another. The mass number of an element is determined by the number of protons and neutrons combined. The atomic number of an element is determined by the number of protons in it, and it is used to differentiate one element from another. The mass number of an element is determined by the number of protons and neutrons combined.

5. Atomic number = number of protons = number of electrons What is Atomic Number? The total number of protons in the nucleus of an atom gives us the atomic number of that atom. It is represented with the letter ‘Z.’ All the atoms of a particular element have the same number of protons, and hence the same atomic number. Atoms of different elements have different atomic numbers. For example, all  carbon atoms  have the atomic number of 6, whereas all atoms of Oxygen have 8 protons in their nucleus. Tuesday, February 2, 20XX Sample Footer Text 5

6. What is Mass Number? The number of protons and neutrons combined to give us the mass number of an atom. It is represented using the letter ‘A.’ As both protons and neutrons are present in the nucleus of an atom, they are together called nucleons. For example, an atom of carbon has 6 protons and 6 neutrons. Thus, its mass number is 12. While the number of protons remains the same in all atoms of an element, the number of neutrons can vary. Thus, atoms of the same element can have different mass numbers, and these are called isotopes. The weight of an electron is almost negligible. Thus, the atomic mass of an atom is almost the same as its mass number. Tuesday, February 2, 20XX Sample Footer Text 6

7. Electrons are a type of subatomic particle with a negative charge. Protons are a type of subatomic particle with a positive charge. Protons are bound together in an atom's nucleus as a result of the strong nuclear force. Neutrons are a type of subatomic particle with no charge (they are neutral). Tuesday, February 2, 20XX Sample Footer Text 7

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9. Tuesday, February 2, 20XX Sample Footer Text 9 All the atoms of an element have the same nuclear charge (atomic number); hence the same number of protons. But experimental evidences have shown that in most cases, the atoms of a given element do not have identical masses. This is so because atoms of the same element may have different numbers of neutrons in their nuclei .  Atoms of an element having the same atomic number, but different mass numbers are called isotopes of that element. Isotopes therefore have the same number of protons and electrons but different number of neutrons.

10. Tuesday, February 2, 20XX Sample Footer Text 10   54 Fe 26                      56 Fe 26          57 Fe 26             58 Fe 26 Shorthand notaion for the naturally occurring isotopes of iron, showing mass number and atomic number A X Z Legend: X = Symbol of an element               A = atomic mass                Z = atomic number Example 32 S 16          Atomic mass = 32           Atomic number = 16

11. Tuesday, February 2, 20XX Sample Footer Text 11 Isotope Element Name Atomic mass Proton Electron Neutron Chanrge Example 1:      Find the number of protons, electrons, and neutrons and charge of the element Nitrogen (N) 14 N 7 N Nitrogen 14 7 7 7 Charge of an element or an isotope is to Subtract proton and electron (p-e)

12. Tuesday, February 2, 20XX Sample Footer Text 12 Elements Atomic Number (Z) Mass Number (A) Proton Electron Neutron Na(Sodium) 11 _________ 11 _________ 12 Ni (Nickel) _________ 59 28 _________ ___________ Ac (Actinum) _________ 227 _________ 89 _________ Cl (Chlorine) 17 _________ _________ _________ 18 Ag (Silver) _________ 108 _________ 47 _________ Using the Periodic Table, fill in the blanks with the information needed to determine the atomic number, atomic mass, number of proton, and electron. APPLICATION-I

13. Tuesday, February 2, 20XX Sample Footer Text 13 APPLICATION-II

14. Tuesday, February 2, 20XX Sample Footer Text 14 Note: Charge of an element or an isotope is to Subtract proton and electron (p-e) Complete the following table below by supplying the information needed for each element.10pts. ASSESSMENT

15. Tuesday, February 2, 20XX Sample Footer Text 15 Make a flashcard of elements with atomic number, mass number, protons, electrons and neutrons. ASSIGNMENT

16. Tuesday, February 2, 20XX Sample Footer Text 16 In determining the number of protons, electron and neutrons, always remember the word "APE MAN"

17. Thank You Cristy R. Villamor- Gesta [email protected] Tuesday, February 2, 20XX Sample Footer Text 17