atomic structure discoveries/experiments conclusions
... Law of Constant Composition (1799, Joseph Proust): “All samples of a compound have the same composition-the same proportions by mass of the constituent elements” ...
... Law of Constant Composition (1799, Joseph Proust): “All samples of a compound have the same composition-the same proportions by mass of the constituent elements” ...
Atomic Structure Guided Notes
... Changes in the number of particles in the nucleus (protons or neutrons) are ______________ ______________. They only take place in ___________________ processes. Electrons have a mass of almost __________________, which means that the mass of each atom results almost entirely from the number of prot ...
... Changes in the number of particles in the nucleus (protons or neutrons) are ______________ ______________. They only take place in ___________________ processes. Electrons have a mass of almost __________________, which means that the mass of each atom results almost entirely from the number of prot ...
Build an Atom
... Depending on the atomic model used, electrons can either be found in _____________or______________. Of the two types of models, the more accurate depiction is the _____________. The atomic number of an element represents the number of each of its atoms contains, which for a neutral atom Is the same ...
... Depending on the atomic model used, electrons can either be found in _____________or______________. Of the two types of models, the more accurate depiction is the _____________. The atomic number of an element represents the number of each of its atoms contains, which for a neutral atom Is the same ...
Chemistry Test #1 Study Guide © Chris Khan
... Diatomic Molecule—contains two atoms; Polyatomic Molecule—more than 2 atoms Ion—atom with + or – charge; Cation—net positive charge; Anion—net negative charge Allotrope—one of two or more distinct forms of an element Organic Compounds have carbon while Inorganic don’t Ionic Compounds—have a metal an ...
... Diatomic Molecule—contains two atoms; Polyatomic Molecule—more than 2 atoms Ion—atom with + or – charge; Cation—net positive charge; Anion—net negative charge Allotrope—one of two or more distinct forms of an element Organic Compounds have carbon while Inorganic don’t Ionic Compounds—have a metal an ...
study guide - atomic srtucture/_classification of matter
... 1-Atom was more than empty space 2-There is a dense portion in the center of the atom that contained most of its mass 3-The nucleus must be positively charged B. Which experiment discovered the electron? cathode ray tube experiment C. Why was the electron discovered first? The theory was that atoms ...
... 1-Atom was more than empty space 2-There is a dense portion in the center of the atom that contained most of its mass 3-The nucleus must be positively charged B. Which experiment discovered the electron? cathode ray tube experiment C. Why was the electron discovered first? The theory was that atoms ...
World of
... 3. Are Malleable (can be hammered into thin sheets) 4. are Ductile (can be drawn into wires) •All metals , except Hg (mercury) are solid at room temperature, 25 ° ...
... 3. Are Malleable (can be hammered into thin sheets) 4. are Ductile (can be drawn into wires) •All metals , except Hg (mercury) are solid at room temperature, 25 ° ...
Homework #1 Atoms
... 1. The number of ____________ in the nucleus of an atom is the atomic ____________ of that element. Because atoms are electrically neutral, the number of protons and ____________ in an atom are equal. 2. The sum of the _____________ and neutrons is the mass number. 3. Atoms of the same element are i ...
... 1. The number of ____________ in the nucleus of an atom is the atomic ____________ of that element. Because atoms are electrically neutral, the number of protons and ____________ in an atom are equal. 2. The sum of the _____________ and neutrons is the mass number. 3. Atoms of the same element are i ...
Structure of the atom
... Calcium-40: mass number = 40; atomic number = 20; number of protons = 20; number of neutrons = 20; number of electrons = 20 (Inquiry point 1) Carbon-14: mass number = 14; atomic number = 6; number of protons = 6; number of neutrons = 8; number of electrons = 6 (Inquiry point 2) Nitrogen-14: mass num ...
... Calcium-40: mass number = 40; atomic number = 20; number of protons = 20; number of neutrons = 20; number of electrons = 20 (Inquiry point 1) Carbon-14: mass number = 14; atomic number = 6; number of protons = 6; number of neutrons = 8; number of electrons = 6 (Inquiry point 2) Nitrogen-14: mass num ...
Here
... However, most elements come in different “species”versions that differ slightly in mass because of having different numbers of neutrons in the nucleus. These “species”of elements are called isotopes. ...
... However, most elements come in different “species”versions that differ slightly in mass because of having different numbers of neutrons in the nucleus. These “species”of elements are called isotopes. ...
Chapter 3: Atoms
... Structure of the Atom A. Atoms consist of two regions: the nucleus, which contains protons and neutrons; and the region surrounding the nucleus, called the electron cloud, where the electrons are. Protons, neutrons, and electrons are also called subatomic particles. 1. Protons - Positively charged p ...
... Structure of the Atom A. Atoms consist of two regions: the nucleus, which contains protons and neutrons; and the region surrounding the nucleus, called the electron cloud, where the electrons are. Protons, neutrons, and electrons are also called subatomic particles. 1. Protons - Positively charged p ...
CHAPTER 5
... elements in order of increasing atomic _____________ and arranging them according to similarities in their properties. He was able to predict the physical and chemical properties of missing elements. In 1913__________________________________, a British physicist, perfected the periodic table by arra ...
... elements in order of increasing atomic _____________ and arranging them according to similarities in their properties. He was able to predict the physical and chemical properties of missing elements. In 1913__________________________________, a British physicist, perfected the periodic table by arra ...
Name ____ Date
... number of protons, neutrons, and electrons in the atoms of different elements. 8. What is the mole and how is the concept used in measuring quantities of an element? 9. How is the periodic table used to determine protons, neutrons, and electrons (especially valence electrons)? 10. What is a group or ...
... number of protons, neutrons, and electrons in the atoms of different elements. 8. What is the mole and how is the concept used in measuring quantities of an element? 9. How is the periodic table used to determine protons, neutrons, and electrons (especially valence electrons)? 10. What is a group or ...
Ch. 4 Slides
... • Protons are the only thing that determines the identity of an atom. • Therefore, it’s possible for atoms of the same element to have different masses due to differing number of neutrons. • isotopes: atoms with the same number of protons, but different numbers of neutrons ...
... • Protons are the only thing that determines the identity of an atom. • Therefore, it’s possible for atoms of the same element to have different masses due to differing number of neutrons. • isotopes: atoms with the same number of protons, but different numbers of neutrons ...
1 An atom is the smallest particle of any element that still retains the
... d) Radiation is absorbed or emitted when an electron moves from one orbit to another. Light of certain colors (and wavelengths) would be created when the electron changed orbits. These postulates were entirely arbitrary but could explain the most of the experiments. ...
... d) Radiation is absorbed or emitted when an electron moves from one orbit to another. Light of certain colors (and wavelengths) would be created when the electron changed orbits. These postulates were entirely arbitrary but could explain the most of the experiments. ...
Ch 3 Notes Atoms
... decimal – is always the larger number on the periodic table. mass number (A) - sum of the protons and neutrons in a nucleus this number is rounded from atomic mass due to the fact that there are isotopes # neutrons = A - Z example - # of neutrons in Li = 6.941-3 = 3.941 rounds to 4 Ion – a charged a ...
... decimal – is always the larger number on the periodic table. mass number (A) - sum of the protons and neutrons in a nucleus this number is rounded from atomic mass due to the fact that there are isotopes # neutrons = A - Z example - # of neutrons in Li = 6.941-3 = 3.941 rounds to 4 Ion – a charged a ...
Chapter 4 Section 1
... chemical symbol for iron. 14. Stars consist of matter in the form of plasma, a gas-like mixture of free electrons and atomic nuclei. 15. Elements are created when the extreme high pressure inside the stars forces atomic nuclei to collide. 16. The process is called nuclear fusion. 17. Nuclear fusion, ...
... chemical symbol for iron. 14. Stars consist of matter in the form of plasma, a gas-like mixture of free electrons and atomic nuclei. 15. Elements are created when the extreme high pressure inside the stars forces atomic nuclei to collide. 16. The process is called nuclear fusion. 17. Nuclear fusion, ...
Nuclear Reactions
... nucleus has too many protons and neutrons Beta Emission- results from conversion of neutron to proton and occurs if nucleus has too many neutrons Positron Emission- results from conversion of proton to neutron and occurs if nucleus has too few neutrons Gamma Emission- often accompanies other decay p ...
... nucleus has too many protons and neutrons Beta Emission- results from conversion of neutron to proton and occurs if nucleus has too many neutrons Positron Emission- results from conversion of proton to neutron and occurs if nucleus has too few neutrons Gamma Emission- often accompanies other decay p ...
Unit #3 Atoms / Atomic Structure / Subatomic Particles
... His experiment involved directing a beam of alpha particles (high energy radiation) at a piece of gold foil. They had expected the radiation to pass straight through the foil. To their surprise, some of it was deflected or ...
... His experiment involved directing a beam of alpha particles (high energy radiation) at a piece of gold foil. They had expected the radiation to pass straight through the foil. To their surprise, some of it was deflected or ...
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.