Atomic Structure - Northwest ISD Moodle
... Protons have a charge of +1 and are located in the nucleus with neutrons. Both are 1,840 times larger than electrons. ...
... Protons have a charge of +1 and are located in the nucleus with neutrons. Both are 1,840 times larger than electrons. ...
atoms
... Rutherford and the Nucleus: Gold Foil Experiment A few particles deflected strongly Some bounced back!! Neutrons (no charge): located in center of atom Protons (+): positively charged particles inside the ...
... Rutherford and the Nucleus: Gold Foil Experiment A few particles deflected strongly Some bounced back!! Neutrons (no charge): located in center of atom Protons (+): positively charged particles inside the ...
Atomic Structure
... Writing the Names of Isotopes • When writing the name of an isotope, you will write the name of the element – the mass number ...
... Writing the Names of Isotopes • When writing the name of an isotope, you will write the name of the element – the mass number ...
File
... Periodic table: A chart in which elements are arranged by increasing atomic number and by changes in physical and chemical properties. atom: The smallest particles that make up matter. proton: a subatomic particle that has a positive charge and that is located in the nucleus of an atom. (The number ...
... Periodic table: A chart in which elements are arranged by increasing atomic number and by changes in physical and chemical properties. atom: The smallest particles that make up matter. proton: a subatomic particle that has a positive charge and that is located in the nucleus of an atom. (The number ...
Atomic Theory Notes Page
... His hypothesis: atoms are eternally unchanging and indivisible (he was not able to prove his thoughts due to lack of technology) o John Dalton Father of Atomic Theory; First to show proof of atoms Experiment: He observed elements combine in whole number ratios to form compounds; Matter is NOT ...
... His hypothesis: atoms are eternally unchanging and indivisible (he was not able to prove his thoughts due to lack of technology) o John Dalton Father of Atomic Theory; First to show proof of atoms Experiment: He observed elements combine in whole number ratios to form compounds; Matter is NOT ...
Atomic Structure
... Scientists use information in the atom to describe elements. The nucleus of an atom has a specific number of protons. This number of protons determines the atom's atomic number and the name of the element. An element's atomic number distinguishes it from other elements. Atoms that are "free" or unch ...
... Scientists use information in the atom to describe elements. The nucleus of an atom has a specific number of protons. This number of protons determines the atom's atomic number and the name of the element. An element's atomic number distinguishes it from other elements. Atoms that are "free" or unch ...
notes ch 39 1st half Atomic Nucleus and Radioactivity
... • Particles only decay when their combined products weigh less than what they started out as. • The mass of a neutron is greater than a decayed neutron (a proton, electron and antineutrino), so there is less mass after decay. ...
... • Particles only decay when their combined products weigh less than what they started out as. • The mass of a neutron is greater than a decayed neutron (a proton, electron and antineutrino), so there is less mass after decay. ...
File - Norris Science
... the tiny alpha particles would pass through the gold atoms and fly straight into the screen. ...
... the tiny alpha particles would pass through the gold atoms and fly straight into the screen. ...
Chem Unit 2 Review Guide ANSWERS
... Atomic mass unit. Equal to the mass of a proton or neutron. 14.) What is a radioactive isotope? An unstable atom which decay (break down) and give off radioactive energy. 15.) What makes an atom unstable? An imbalance in the ratio of protons to neutrons. The farther this ratio gets from 1:1, the mor ...
... Atomic mass unit. Equal to the mass of a proton or neutron. 14.) What is a radioactive isotope? An unstable atom which decay (break down) and give off radioactive energy. 15.) What makes an atom unstable? An imbalance in the ratio of protons to neutrons. The farther this ratio gets from 1:1, the mor ...
Chapter 21 - Richsingiser.com
... 4 Certain numbers of protons and neutrons (called magic numbers) confer unusual stability: 2, 8, 20, 26, 28, 50, 82, and 126. 5 The zone of stability contains all of the stable nuclides, but some nuclides in this band are unstable. 6 Tc (Z=43), Pm (Z=61), and all elements beyond Bi (Z=83) have no st ...
... 4 Certain numbers of protons and neutrons (called magic numbers) confer unusual stability: 2, 8, 20, 26, 28, 50, 82, and 126. 5 The zone of stability contains all of the stable nuclides, but some nuclides in this band are unstable. 6 Tc (Z=43), Pm (Z=61), and all elements beyond Bi (Z=83) have no st ...
the Atom
... 2. Compare and contrast the properties of electrons, neutrons and protons. 3. Distinguish between atomic number and mass number. 4. Use atomic number and mass number to distinguish between isotopes. 5. Using the concept of isotopes, explain why atomic masses of elements are not whole numbers. 6. Dis ...
... 2. Compare and contrast the properties of electrons, neutrons and protons. 3. Distinguish between atomic number and mass number. 4. Use atomic number and mass number to distinguish between isotopes. 5. Using the concept of isotopes, explain why atomic masses of elements are not whole numbers. 6. Dis ...
Atomic Structure/Electrons
... 6. An atom is defined as the smallest part of an element that: a. contains at least one proton, neutron and electron. b. retains the chemical identity of the element. c. can carry an electrical charge. d. is affected in a cathode ray tube. 7. The electrical charges in an atom are located: a. only in ...
... 6. An atom is defined as the smallest part of an element that: a. contains at least one proton, neutron and electron. b. retains the chemical identity of the element. c. can carry an electrical charge. d. is affected in a cathode ray tube. 7. The electrical charges in an atom are located: a. only in ...
Finding the Amounts of Subatomic Particles
... ◦ Mass of 1 atomic mass unit (AMU). ◦ Discovered by Ernest Rutherford in 1911. ...
... ◦ Mass of 1 atomic mass unit (AMU). ◦ Discovered by Ernest Rutherford in 1911. ...
Atomic Theory- 1. Matter is composed of tiny, indivisible particles
... Atomic Theory1. Matter is composed of tiny, indivisible particles called atoms. 2. An element is composed of one type of atom. Properties of atoms are identical to each other. 3. A compound contains two or more different elements. The relative number of atoms of each element in a compound is the sam ...
... Atomic Theory1. Matter is composed of tiny, indivisible particles called atoms. 2. An element is composed of one type of atom. Properties of atoms are identical to each other. 3. A compound contains two or more different elements. The relative number of atoms of each element in a compound is the sam ...
Average Atomic Mass
... Average atomic mass • Definition: Weighted atomic masses of the isotopes of each element • Each isotope has a known natural occurrence (percentage of that elements’ atoms) ...
... Average atomic mass • Definition: Weighted atomic masses of the isotopes of each element • Each isotope has a known natural occurrence (percentage of that elements’ atoms) ...
Chem. Review Notes
... Mass number • each proton and each neutron has a mass of 1 atomic mass unit (amu) • mass number is number of protons plus number of neutrons • e.g. an atom has 6 protons and 6 neutrons – its mass number is 6 + 6 = 12 amu – what element is this? ...
... Mass number • each proton and each neutron has a mass of 1 atomic mass unit (amu) • mass number is number of protons plus number of neutrons • e.g. an atom has 6 protons and 6 neutrons – its mass number is 6 + 6 = 12 amu – what element is this? ...
Ch 21.1 Study Guide
... 1. _____ Based on the information about the three elementary particles on page 683 of the text, which has the greatest mass? (a) the proton (b) the neutron (c) the electron (d) They all have the same mass. 2. _____ The force that keeps nucleons together is (a) a strong nuclear force. (b) a weak nucl ...
... 1. _____ Based on the information about the three elementary particles on page 683 of the text, which has the greatest mass? (a) the proton (b) the neutron (c) the electron (d) They all have the same mass. 2. _____ The force that keeps nucleons together is (a) a strong nuclear force. (b) a weak nucl ...
Isotope
Isotopes are variants of a particular chemical element which differ in neutron number, although all isotopes of a given element have the same number of protons in each atom. The term isotope is formed from the Greek roots isos (ἴσος ""equal"") and topos (τόπος ""place""), meaning ""the same place""; thus, the meaning behind the name it is that different isotopes of a single element occupy the same position on the periodic table. The number of protons within the atom's nucleus is called atomic number and is equal to the number of electrons in the neutral (non-ionized) atom. Each atomic number identifies a specific element, but not the isotope; an atom of a given element may have a wide range in its number of neutrons. The number of nucleons (both protons and neutrons) in the nucleus is the atom's mass number, and each isotope of a given element has a different mass number.For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14 respectively. The atomic number of carbon is 6, which means that every carbon atom has 6 protons, so that the neutron numbers of these isotopes are 6, 7 and 8 respectively.