Inside the Atom 1. Atom – greek for cannot be divided. Democritus
... a. In the 1800s, scientists discovered that all matter is made up of elements either in pure form Au, Ag or Fe, or in combinations such as the molecules of H2O & NaCl b. 1st Model: Dalton – proposed that the atom was a hard sphere which was the same all the way through. Dalton’s idea of what atoms ...
... a. In the 1800s, scientists discovered that all matter is made up of elements either in pure form Au, Ag or Fe, or in combinations such as the molecules of H2O & NaCl b. 1st Model: Dalton – proposed that the atom was a hard sphere which was the same all the way through. Dalton’s idea of what atoms ...
protons and neutrons
... Most of the particles passed right through A few particles were deflected VERY FEW were greatly deflected ...
... Most of the particles passed right through A few particles were deflected VERY FEW were greatly deflected ...
Properties of Atoms and the Periodic Table
... Directions: Complete the concept map using the terms in the list below. Terms can be used more than once, protons ...
... Directions: Complete the concept map using the terms in the list below. Terms can be used more than once, protons ...
5.7 Nuclear Radiation
... – The process continues until unstable isotopes of one element are changed, or transformed, into stable isotopes of a different element. – These stable isotopes are not radioactive. – Nuclear radiation is emitted during radioactive decay. – There are three main types of nuclear radiation: alpha rad ...
... – The process continues until unstable isotopes of one element are changed, or transformed, into stable isotopes of a different element. – These stable isotopes are not radioactive. – Nuclear radiation is emitted during radioactive decay. – There are three main types of nuclear radiation: alpha rad ...
2-1 Chemistry of life
... energy levels of the six electrons in a carbon atom. Carbon will have 2 electrons in the first energy level and four electrons in the second level How many valence electrons does carbon have to share with other atoms? ...
... energy levels of the six electrons in a carbon atom. Carbon will have 2 electrons in the first energy level and four electrons in the second level How many valence electrons does carbon have to share with other atoms? ...
Mass Defect (not in book)
... the nucleus. This number is what gives an element its identity. For example, any atom with 6 protons in its nucleus is carbon. The periodic table is arranged in order of increasing atomic number. Mass Number Atoms of the same element can differ in the number of neutrons in the nucleus. Such variatio ...
... the nucleus. This number is what gives an element its identity. For example, any atom with 6 protons in its nucleus is carbon. The periodic table is arranged in order of increasing atomic number. Mass Number Atoms of the same element can differ in the number of neutrons in the nucleus. Such variatio ...
Chapter 18 Notes
... atomic theory—states that all matter is composed of tiny particles called atoms o John Dalton was one of the first scientists to gather evidence for the atomic theory o Dalton’s Atomic Theory: • Each element is composed of atoms • All atoms of a given element are identical • Atoms of different eleme ...
... atomic theory—states that all matter is composed of tiny particles called atoms o John Dalton was one of the first scientists to gather evidence for the atomic theory o Dalton’s Atomic Theory: • Each element is composed of atoms • All atoms of a given element are identical • Atoms of different eleme ...
Atomic Structure Summary Sheet
... 1. If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ra ...
... 1. If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ra ...
Getting to Know: Periodic Table
... Misconception: Why is the atomic mass defined as the “average” mass of atoms of an element? Aren’t all atoms of the same element identical? All atoms of the same element have the same number of protons. All atoms of the same element do not have the same number of neutrons. For example, most atoms of ...
... Misconception: Why is the atomic mass defined as the “average” mass of atoms of an element? Aren’t all atoms of the same element identical? All atoms of the same element have the same number of protons. All atoms of the same element do not have the same number of neutrons. For example, most atoms of ...
notes 4.1 & 4.2
... Do we have to know this? • But you’ll hear more about that in chemistry. For now realize that each energy level is made up of sublevels that hold specific amounts of electrons. • The sublevels are called orbitals and are named s, p, d, f • You can see these patterns in the periodic table. ...
... Do we have to know this? • But you’ll hear more about that in chemistry. For now realize that each energy level is made up of sublevels that hold specific amounts of electrons. • The sublevels are called orbitals and are named s, p, d, f • You can see these patterns in the periodic table. ...
Chapter 4: Atomic Structure
... then the protons that account for the positive charge do not account for the total mass – only part of it. 6. Therefore, the atom had more mass than the amount contributed by the protons. 7. Suggested tightly bound proton-electron pairs which he called neutrons to account for the missing mass – no r ...
... then the protons that account for the positive charge do not account for the total mass – only part of it. 6. Therefore, the atom had more mass than the amount contributed by the protons. 7. Suggested tightly bound proton-electron pairs which he called neutrons to account for the missing mass – no r ...
Bohr´s atomic model (1913)
... The mass number is not necessarily the same in all the atoms of an element, because the number of neutrons can change in an element. Atoms with the same Z (therefore of the same element) and with different A (therefore with different number of neutrons) are called isotopes. ...
... The mass number is not necessarily the same in all the atoms of an element, because the number of neutrons can change in an element. Atoms with the same Z (therefore of the same element) and with different A (therefore with different number of neutrons) are called isotopes. ...
NUCLEAR CHEMISTRY
... Shielding – radiation-absorbing material used to decrease the emission of radiation, especially gamma rays, from nuclear reactors. Control rods – neutron-absorbing rods that help control the reaction by limiting free neutrons. Moderator – used to slow down the fast neutrons produced by fission Urani ...
... Shielding – radiation-absorbing material used to decrease the emission of radiation, especially gamma rays, from nuclear reactors. Control rods – neutron-absorbing rods that help control the reaction by limiting free neutrons. Moderator – used to slow down the fast neutrons produced by fission Urani ...
study guide for atoms/periodic table quiz
... Period ROWS in the Periodic Table are called periods. The elements in a period have very different properties. Family/Group COLUMNS in the Periodic Table represent groups or families. Elements in the same family have similar properties. Bohr Diagram A drawing which shows electrons in their energy le ...
... Period ROWS in the Periodic Table are called periods. The elements in a period have very different properties. Family/Group COLUMNS in the Periodic Table represent groups or families. Elements in the same family have similar properties. Bohr Diagram A drawing which shows electrons in their energy le ...
Chapter 3
... Isotopes: atoms of the same element (X) with different numbers of neutrons in their nuclei ...
... Isotopes: atoms of the same element (X) with different numbers of neutrons in their nuclei ...
Atom Review
... Postulates 1-4 (pg. 92 in book) 1. Each element is composed of extremely small particles called atoms. 2. All atoms of a given element are identical, but they differ from those of any other element. 3. Atoms are neither created nor destroyed in any chemical reaction. They are dissociated, combined o ...
... Postulates 1-4 (pg. 92 in book) 1. Each element is composed of extremely small particles called atoms. 2. All atoms of a given element are identical, but they differ from those of any other element. 3. Atoms are neither created nor destroyed in any chemical reaction. They are dissociated, combined o ...
NUCLEAR CHEMISTRY
... normally strong enough to hold the protons and neutrons together. However, sometimes the force of repulsion due to the protons having the same charge overcomes the strong nuclear force and the atom breaks apart. ...
... normally strong enough to hold the protons and neutrons together. However, sometimes the force of repulsion due to the protons having the same charge overcomes the strong nuclear force and the atom breaks apart. ...
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.