UNIT 1: ATOMIC STRUCTURE & PROPERTIES
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46 Terms
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Electronegativity
how strongly the nucleus of an atom attracts the electrons of other atoms in a bond.
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Hunds Rule
when an electron is added to a subshell, it will always occupy an empty orbital if one is available.
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important information
The periodic table gives you basic but ________ about each element.
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Subshells
________- a subdivision of electron shells separated by orbitals (s, p, d, & f)
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Orbital
________- the position surrounding an atoms nucleus where electrons are most likely to be found at any given moment.
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Energy Level
________- fixed distances from the nucleus of an atom where electrons may be found (1- 7)
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Isotopes
Atoms of an element with different number of neutrons.
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Molarity
(M)- moles of solute /liters of solution.
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Aufbau Principle
when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy.
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Electron Affinity
the energy change that occurs when an electron is added to an atom in its gaseous state.
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Pauli Exclusion Principle
two electrons which share an orbital can not have the same spin.
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Electrostatic Force
the attraction between opposite charges.
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Symbol
The unique symbol that represents an element on the periodic table.
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Ionization Energy
the energy required to remove an electron from an atom.
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Mass Number
The sum of an atoms protons and neutrons.
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Valence Electrons
the electrons in the outermost s and p subshells.
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Avogadros Number
The number of atoms that are in a single mole of any given element (6.022 x 10^23 particles)
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Atomic Radius
the approximate distance from the nucleus of an atom to its valence electrons.
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Empirical Formula
The simplest ratio of one element to another in a compound.
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Symbol
The unique symbol that represents an element on the periodic table
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Atomic Number
The number of protons located within the nucleus of an element
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Molar Mass
The average atomic mass of an atom and also the average mass per mol of the atom
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Periods
the horizontal rows of the periodic table
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Groups
the vertical columns of the periodic table
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The two rows offset beneath the table are alternatively called the Lanthanides (4f) and the Actinides (5f)
Rare Earth Metals or Inner Transition Metals
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Mass Number
The sum of an atoms protons and neutrons
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Isotopes
Atoms of an element with different number of neutrons
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Avogadros Number
The number of atoms that are in a single mole of any given element (6.022 x 10^23 particles)
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Molarity(M)
moles of solute/liters of solution
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Empirical Formula
The simplest ratio of one element to another in a compound
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Molecular Formula
The actual formula for a substance
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Electrostatic Force
the attraction between opposite charges
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Coulombs Law
Force of attraction = q1q2/r^2
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Energy Level
fixed distances from the nucleus of an atom where electrons may be found (1-7)
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Subshells
a subdivision of electron shells separated by orbitals (s, p, d, & f)
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Orbital
the position surrounding an atoms nucleus where electrons are most likely to be found at any given moment
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Electron Configuration
the complete description of the energy level and subshell that each electron on an element inhabits
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Aufbau Principle
when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy
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Pauli Exclusion Principle
two electrons which share an orbital cannot have the same spin
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Hunds Rule
when an electron is added to a subshell, it will always occupy an empty orbital if one is available
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Valence Electrons
the electrons in the outermost s and p subshells
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Atomic Radius
the approximate distance from the nucleus of an atom to its valence electrons
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Ionization Energy
the energy required to remove an electron from an atom
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Electronegativity
how strongly the nucleus of an atom attracts the electrons of other atoms in a bond
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Electron Affinity
the energy change that occurs when an electron is added to an atom in its gaseous state
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Effective Nuclear Charge
The net attractive force of the nucleus on the valence electrons (approximately equal to the number of protons - core electrons)
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