![atom - Images](http://s1.studyres.com/store/data/008518465_1-b79e76edc81afcc909029e7609767c9b-300x300.png)
Specific Objectives:
... n = principal quantum number. As the Bohr quantum number it roughly describes the distance of the electron from the nucleus of an atom. It may have the integral values of 1, 2, 3, 4, … infinity. l = azimuthal or angular momentum quantum number. This quantum number describes the shape of the orbital. ...
... n = principal quantum number. As the Bohr quantum number it roughly describes the distance of the electron from the nucleus of an atom. It may have the integral values of 1, 2, 3, 4, … infinity. l = azimuthal or angular momentum quantum number. This quantum number describes the shape of the orbital. ...
chapter 2 - WorkNotes
... groups or families--vertical columns; have similar physical and chemical properties (based on similar electron configurations!!) ...
... groups or families--vertical columns; have similar physical and chemical properties (based on similar electron configurations!!) ...
Name: Date: Chemistry 1 – Midterm Review Sheet Unit 1 – Scientific
... 11. Halogens exist naturally as these types of molecules. e. Monatomic f. Diatomic g. Elements h. Ionic 12. Which of the following elements is most chemically similar to Ca? a. Na b. N c. O d. Mg e. C 13. Rows of the periodic table are called? _________Periods___________________________ 14. Columns ...
... 11. Halogens exist naturally as these types of molecules. e. Monatomic f. Diatomic g. Elements h. Ionic 12. Which of the following elements is most chemically similar to Ca? a. Na b. N c. O d. Mg e. C 13. Rows of the periodic table are called? _________Periods___________________________ 14. Columns ...
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 ...
Physical Science Chapter 1
... Suppose that you have discovered a new element and have named it neptunite. While studying your new element, you find that it has two isotopes –neptunite220 and neptunite-250. What is the average atomic mass of your new element assuming that these two ...
... Suppose that you have discovered a new element and have named it neptunite. While studying your new element, you find that it has two isotopes –neptunite220 and neptunite-250. What is the average atomic mass of your new element assuming that these two ...
atomic models
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
PowerPoint - Models of the Atom
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
Workshop - History of Atomic Theory
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
Foldable - Georgetown ISD
... Ions: when an atom has lost or gained electrons it becomes an ion. Ions have either a positive or negative charge. Atoms do not have a charge because in an ATOM the #protons = #electrons. To calculate the charge of an ion = #protons - #electrons Example: Write the nuclear symbol for an ion with 10 e ...
... Ions: when an atom has lost or gained electrons it becomes an ion. Ions have either a positive or negative charge. Atoms do not have a charge because in an ATOM the #protons = #electrons. To calculate the charge of an ion = #protons - #electrons Example: Write the nuclear symbol for an ion with 10 e ...
Electrons
... the elements in the second row (the second period) have two orbitals for their electrons. It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven. ...
... the elements in the second row (the second period) have two orbitals for their electrons. It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven. ...
ATOM
... • The horizontal rows of the periodic table are called periods • A row is called a period because the properties of elements in a row follow a repeating, or periodic, pattern • The elements in a row become less metallic from left to right • The row number indicates the number of “rings” (energy leve ...
... • The horizontal rows of the periodic table are called periods • A row is called a period because the properties of elements in a row follow a repeating, or periodic, pattern • The elements in a row become less metallic from left to right • The row number indicates the number of “rings” (energy leve ...
Solute
... Every element has a unique atomic number Atomic number – number of protons in the nucleus ...
... Every element has a unique atomic number Atomic number – number of protons in the nucleus ...
Atoms and Atomic Structure Learning Targets
... Define and explain what the atomic mass unit of an atom is. Identify the mass of each sub-atomic particle. Identify the electric charge of each sub-atomic particle. Identify the location of each sub-atomic particle in the atom. Describe the nucleus of an atom and what makes it up. Identify how to de ...
... Define and explain what the atomic mass unit of an atom is. Identify the mass of each sub-atomic particle. Identify the electric charge of each sub-atomic particle. Identify the location of each sub-atomic particle in the atom. Describe the nucleus of an atom and what makes it up. Identify how to de ...
Atom
... explain this. Bohr suggested that the electrons must be orbiting the nucleus in certain fixed energy levels (or shells). The nucleus is the centre of an atom, containing protons and neutrons. The energy must be given out when 'excited' electrons fall from a high energy level to a low one. ...
... explain this. Bohr suggested that the electrons must be orbiting the nucleus in certain fixed energy levels (or shells). The nucleus is the centre of an atom, containing protons and neutrons. The energy must be given out when 'excited' electrons fall from a high energy level to a low one. ...
Atomic Structure
... 1) Elements composed of tiny indivisible (not invisible) particles called atoms 2) Atoms of the same element are identical 3) Atoms of different elements can chemically combine with one another in simple whole number ratios (compounds) 4) In chemical reactions, atoms are separated, joined, a ...
... 1) Elements composed of tiny indivisible (not invisible) particles called atoms 2) Atoms of the same element are identical 3) Atoms of different elements can chemically combine with one another in simple whole number ratios (compounds) 4) In chemical reactions, atoms are separated, joined, a ...
Chemistry powerpoint notes
... the elements in the second row (the second period) have two orbitals for their electrons. It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven. ...
... the elements in the second row (the second period) have two orbitals for their electrons. It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven. ...
Periodic table
The periodic table is a tabular arrangement of the chemical elements, ordered by their atomic number (number of protons in the nucleus), electron configurations, and recurring chemical properties. The table also shows four rectangular blocks: s-, p- d- and f-block. In general, within one row (period) the elements are metals on the lefthand side, and non-metals on the righthand side.The rows of the table are called periods; the columns are called groups. Six groups (columns) have names as well as numbers: for example, group 17 elements are the halogens; and group 18, the noble gases. The periodic table can be used to derive relationships between the properties of the elements, and predict the properties of new elements yet to be discovered or synthesized. The periodic table provides a useful framework for analyzing chemical behavior, and is widely used in chemistry and other sciences.Although precursors exist, Dmitri Mendeleev is generally credited with the publication, in 1869, of the first widely recognized periodic table. He developed his table to illustrate periodic trends in the properties of the then-known elements. Mendeleev also predicted some properties of then-unknown elements that would be expected to fill gaps in this table. Most of his predictions were proved correct when the elements in question were subsequently discovered. Mendeleev's periodic table has since been expanded and refined with the discovery or synthesis of further new elements and the development of new theoretical models to explain chemical behavior.All elements from atomic numbers 1 (hydrogen) to 118 (ununoctium) have been discovered or reportedly synthesized, with elements 113, 115, 117, and 118 having yet to be confirmed. The first 94 elements exist naturally, although some are found only in trace amounts and were synthesized in laboratories before being found in nature. Elements with atomic numbers from 95 to 118 have only been synthesized in laboratories. It has been shown that einsteinium and fermium once occurred in nature but currently do not. Synthesis of elements having higher atomic numbers is being pursued. Numerous synthetic radionuclides of naturally occurring elements have also been produced in laboratories.