vocabulary atomic structure. anion ___ are negatively charged ions - atoms that take electrons
TRANSCRIPT
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Vocabulary
Atomic Structure
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anion
• ___ are negatively charged ions - atoms that take electrons.
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atomic number
• ____ is equal to the number of protons in an atom; used to arrange the periodic table.
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Aufbau Principle
• The _____ tells us that electrons fill the energy levels from the nucleus out.
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average atomic mass
• By taking the weighted percentage of all naturally occurring isotopes of an element, we can calculate the ____, which is the mass found on the periodic table.
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Bohr's Atomic Model• ____ of an atom is a simplified visual
representation of invisible atomic structures, where the nucleus is surrounded by layers of electron shells that allow us to visualize something that is too small to be seen.
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cation
• ____ are positively charged ions - atoms that give away electrons.
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charge• Atoms that give or take electrons
and become ions are said to have a positive or negative ____, which causes them to attract or repel other particles that have a ____similar to a magnet (same word in both blanks).
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Dalton's Postulates
• In the early 1800's, ___ were published, which gave us a strong definition for nuclear theory, much of which is upheld today.
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electron
• ___ are subatomic particles with a negative charge, no mass value, and are located outside the nucleus of the atom; responsible for chemical reactions.
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electron cloud
• The area of an atom that holds the electrons is called the ___, which is divided into levels and sublevels called orbitals.
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electron configuration• ____ is a representation of how the
electrons are grouped or stacked around the nucleus of an atom. It can be drawn out in picture form (orbital diagram) using arrows, or in a shorter version, only naming the sublevels and the number of electrons present in each.
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electron shell
• An orbital or sublevel is sometimes called an ____, with the very outer one being called the valence shell.
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energy
• ___ is the ability or capacity to do work or to produce change. Forms include heat, light, sound, electricity, and chemical energy.
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energy levels
• For electron configuration, the electron shells are grouped into ___.
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Hund's Rule
• _______ demonstrates that electrons must fill the energy levels / orbitals evenly - they will spread out before they share in a level.
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hyphen notation
• ___ gives the name of the element and the number of the atomic mass separated by a hyphen - such as carbon-12.
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ions
• ____ are the result of gaining or losing electrons by atoms.
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isotopes
• Atoms have different numbers of neutrons in their nuclei, which are said to be ____ because their masses will vary.
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Lewis Dot Diagram
• A ___ is used to depict how many valence electrons surround a given atom by using the nuclear symbol surrounded by the proper number of dots.
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mass number
• ___ is equal to protons plus neutrons; it is the average atomic mass rounded to a whole number.
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neutron
• A ___ is a subatomic particle with no charge, mass is about 1, and is located in the nucleus of an atom.
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nuclear symbol
• The letter or letters that represent an element are called the _____, which can include details about the structure or parts of that atom.
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octet rule• The _____ tells us that all atoms want
to have 8 electrons in their valence shell, with H as an exception. (Remember that all atoms can only hold 2 electrons in the very first energy level, which is the only completely stable exception to this rule)
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orbital
• The exact 'mini highway' that electrons fly around on is called an ___.
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orbital diagram
• When showing the how the electrons are grouped or stacked around the nucleus of an atom, It can be drawn out in picture form called an _____ using arrows, or in a shorter version, only naming the sublevels and the number of electrons present in each.
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Pauli Exclusion Principle
• The ______ states that there can only be 2 or less electrons in each orbital of each energy level and they must have opposite spins.
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proton
• A subatomic particle with a positive charge is called a ____, has mass of about 1, and is located in the nucleus of the atom.
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Rutherford's Atomic Model
• ____ of the atom describes it as a small, heavy nucleus surrounded by orbital electrons; this was the basis for other scientists who completed the model to represent atoms in the way they are understood to exist still today.
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Schrodinger & quantum mechanic model
• ___ attempt to explain the structure of an atom and electron configuration by using the laws of probability to predict the location of electrons.
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subatomic particles
• The parts that make up an atom are called ____ - protons, neutrons and electrons.
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sublevels
• When describing electron configuration, remember that each level is broken down into ____, called s, p, d and f, each with a specific number of orbitals.
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Thomson's Experiments• In ____, he used a cathode ray to
determine charges and locations of subatomic particles. His theory (called the 'plum pudding model’) was later disproved, but did serve as a strong catalyst for the work of others.
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valence
• The outer energy level of an atom is called the ____ shell and the electrons that are in it are called ____ electrons. (same word for both blanks).