Introduction: The information provided on the periodic table allows you to determine the number of protons, neutrons, and electrons in any given atom of an element. The atomic number is always equal to the number of protons. The number of electrons is equal to the number of protons. And the number of neutrons is equal to the difference between the mass number and the atomic number. *Remember: A=P3DE and M-A=N* Element name- Mercury 80 Atomic # Symbol > Hg 200.59 < Avg. Mass Directions: Using the periodic table, determine the atomic number, mass number, and number of protons, neutrons and electrons in an atom of each of the following fifteen elements. 1. Boron a. Atomic N: Mass N: Protons: Electrons: Neutrons: 2. Copper a. Atomic N: Mass N: Protons: Electrons: Neutrons: 3. Lead a. Atomic N: Mass N: Protons: Electrons: Neutrons: 4. Hydrogen a. Atomic N: Mass N: Protons: Electrons: Neutrons:

Introduction: The information provided on the periodic table allows you to determine the number of protons, neutrons, and electrons in any given atom of an element. The atomic number is always equal to the number of protons. The number of electrons is equal to the number of protons. And the number of neutrons is equal to the difference between the mass number and the atomic number. Remember: A=P3DE and M-A=N Element name- Mercury 80 Atomic # Symbol > Hg 200.59 < Avg. Mass Directions: Using the periodic table, determine the atomic number, mass number, and number of protons, neutrons and electrons in an atom of each of the following fifteen elements. 1. Boron a. Atomic N: Mass N: Protons: Electrons: Neutrons: 2. Copper a. Atomic N: Mass N: Protons: Electrons: Neutrons: 3. Lead a. Atomic N: Mass N: Protons: Electrons: Neutrons: 4. Hydrogen a. Atomic N: Mass N: Protons: Electrons: Neutrons:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter4: Chemical Foundations: Elements, Atoms, And Ions

Section: Chapter Questions

Problem 95AP: Though the common isotope of aluminum has a mass number of 27, isotopes of aluminum have been...

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2-27 If each atom in Problem 2-26 acquired two more neutrons, what element would each then be?
Do the proton and the neutron have exactly the same mass? How do the masses of the proton and neutron compare to the mass of the electron? Which particles make the greatest contribution to the mass of an atom? Which particles make the greatest contribution to the chemical properties of an atom?
2.87 What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must he true about the nuclei of atoms with higher atomic numbers?
Give the atomic number (Z) and the mass number (A) for each of the following: a. a carbon atom with 8 neutrons b. an aluminum atom with 14 neutrons c. an argon atom with 20 neutrons d. a copper atom with 36 neutrons
Give the complete symbol(ZAX), including atomic number and mass number, of (a) a nickel atom with 31 neutrons, (b) a plutonium atom with 150 neutrons, and (c) a tungsten atom with 110 neutrons.
How many protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, how many electrons are present? a.56130Ba c .2246Ti e.36Li b.56136Ba d.2248Ti f.37Li
Though the common isotope of aluminum has a mass number of 27, isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of 24, 25, 26, 28, 29, and 30. How many neutrons are present in each of these isotopes? Why are they all considered aluminum atoms, even though they differ greatly in mass? Write the atomic symbol for each isotope.
How many protons and neutrons are contained in the nucleus of each of the following atoms? In an atom of each element, how many electrons are present? a.2241Ti d.3686Kr b.3064Zn e.3375As c.3276Ge f.1941K
2.13 How many electrons, protons, and neutrons are there in each of the following atoms? (a) 24Mg, (b) 119Sn, (c) 232Th, (d) 13C, (e) 63Cu, (f) 205Bi
A single molecule has a mass of 7.31 1023 g. Provide an example of a real molecule that can have this mass. Assume the elements that make up the molecule are made of light isotopes where the number of protons equals the number of neutrons in the nucleus of each element.
Which pair of elements do you expect to be most similar? a. Mg and Ca b. N and Cl c. Al and C d. S and Si
Calculate the atomic mass of each of the following elements using the given data for the percentage abundance and mass of each isotope. a. Lithium: 7.42% 6Li (6.01 amu) and 92.58% 7Li (7.02 amu) b. Magnesium: 78.99% 24Mg (23.99 amu), 10.00% 25Mg (24.99 amu), and 11.01% 26Mg (25.98 amu)