Review for Chem110 quiz/test for DelTech Owens
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| What is the basic structural unit of an element? | The atom
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| An atom is the smallest unit of an element that retains the __ of that element. | properties
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| What are the 3 primary particles of an atom? | electrons, protons, neutrons
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| A small, dense, positively charged region in the center of an atom is called the __. | nucleus
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| Protons are __ charged. | positively
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| Neutrons have a __ charge. | neutral
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| Electrons have a __ charge. | negative
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| If the electrons and protons of an atom are equal in number, the atom will have a __ charge. | neutral
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| On the periodic table, the number of protons in an atom is represented by the __ __. | atomic number
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| On the periodic table, the sum of the protons and neutrons is called the __ __. | mass number
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| On the periodic table, if there is no charge shown for an element, then its charge is __. | zero
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| To find the number of electrons for an element on the periodic table, subtract the __ __ from the __ __. | mass number from the atomic number
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| What is the mass and charge for an electron? | Charge = -1; Mass (amu)= 5.4 x 10^-28
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| Electrons are abbreviated as __. | e
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| What is the mass and charge for a proton? | Charge = +1; Mass (amu) = 1.00
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| Protons are abbreviated as __. | p
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| What is the mass and charge for a neutron? | Charge = 0; Mass (amu) = 1.00
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| Neutrons are abbreviated as __. | n
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| Atoms of the same element that have different masses than the "normal" atom of that element are called __. | isotopes
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| Isotopes contain the same number of __ as a normal atom of that element. | protons
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| Isotopes have __ __ number of __. | a different number of neutrons
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| Two isotopes of hydrogen are called __ and __. | deuterium and tritium
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| Isotopes of the same element have __ chemical properties. | identical
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| Some isotopes are __. | radioactive
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| The atomic mass is really the __ __ of the masses of all the isotopes that make up the element. | weighted average
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| An average corrected by the relative amounts of each isotope present in nature is called the __ __. | weighted average (which is equal to its atomic mass)
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| The first experimentally based theory of atomic structure is called __ __ __. | Dalton's Atomic Theory
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| Which of Dalton's Atomic Theory postulates is wrong? | 2 and 3; the rest are all true.
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| What disproves the following postulate from Dalton's Atomic Theory (#2): "An atom cannot be created, divided, destroyed, or converted to any other type of atom." | radioactivity
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| What disproves the following postulate from Dalton's Atomic Theory (#3): "Atoms of a particular element have identical properties." | isotopes
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| Thomson (of Crookes and Thomson) discovered the __. | electron
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| Electrons were the first subatomic particle to be discovered. This was done using a __ __ __. | cathode ray tube
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| Experiments by __ __ and __ __ showed that the atom is composed of + and - particles. | William Crookes and Eugene Goldstein
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| When Crookes ran his experiment using a cathode ray tube, rays of lights were seen traveling between the two electrodes. The electrodes were called the __ and the __. | cathode, anode
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| The cathode in a cathode ray tube was __ (negative or positive)? | negative
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| The anode in a cathode ray tube was __ (negative or positive)? | positive
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| Later experiments by __ proved the rays were both electrical and magnetic. | J.J. Thomson
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| The ability to produce cathode rays is a characteristic of __ __. | all materials
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| It was Thomson who announced that cathode rays were really streams of negative particles of energy. These particles are __. | electrons
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| Experiments by Goldstein proved that there were particles of equal charge, but of opposite sign, to the electron. Those particles are called __. | protons
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| Neutrons have a mass almost __ to that of a proton. | identical
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| The mass of a neutron is __ __ __ __ lower than that of a proton. | less than 1%
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| Neutrons were proven to exist by __ __. | James Chadwick
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| Rutherford's __ __ experiment proved that the atom is mostly empty space. | Gold Foil
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| We use the measurement of particle __ rather than position. | energy
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| The absorption or emission of light by atoms is called __. | spectroscopy
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| Spectroscopy is used to understand the electronic __. | structure
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| Light is a form of __ __. | electromagnetic radiation
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| Electromagnetic radiation travels in __ from a source. | waves
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| The speed of light is __. | 3.0 x 10^8 m/s
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| Electromagnetic radiation goes farther if its __ are shorter. | waves
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| Light moves as a collection of __ waves. | sine
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| The distance between identical points on successive waves is called __. | wavelength
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| Each wavelength of electromagnetic radiation travels at the same __ but has its own characteristic energy. | velocity
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| Wavelengths and energy are __ related when talking about electromagnetic radiation. | inversely
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| Bohr's theory: atoms can absorb and emit energy via __ of electrons to higher energy levels. | promotion
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| Bohr's theory: when excited electrons return to lower levels of energy, this is called __. | relaxation
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| Bohr's theory: __ __ are a result of electron transitions between __ __ in the atoms. | allowed levels
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| Each electron has its own __ lines, or signature. | spectral
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| Each element has its own __ __. | electron structure
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| Spectral lines of electrons can be seen using a __. | spectroscope
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| The emission spectrum of what element lead to the modern understanding of the electronic structure of the atom? | hydrogen
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| Bohr's Atom: electrons exist in fixed energy levels surrounding the __. | nucleus
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| Bohr's Atom: promotion of electrons occurs as they absorb __. | energy
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| Bohr's Atom: energy is released as an electron travels back to __ __ once its excess energy has been used. | lower levels; this is called relaxation
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| Bohr's Atom: the amount of energy absorbed when an electron jumps from one energy level to a higher energy level is a __ quantity. | precise
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| Bohr's Atom: when an electron jumps from one energy level to a higher one, the difference between the orbits represents the __ of that jump. | energy
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| Bohr called the fixed energy levels of electrons __. | orbits
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| Bohr called the lowest possible energy level for an electron its __ __. | ground state
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| According to Bohr's theory, electrons are only found in __ levels, or obits. | allowed
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| An electron's orbit is different from an atomic __. | orbital
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| One major change between Bohr's Atomic Theory and modern Atomic Theory is that electrons do not move in __. | orbits
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| Bohr's model of the atom failed to explain their line __. | spectra
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| Electrons move rapidly within the atomic orbital giving it a high __ __. | electron density
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| The Periodic Table was invented independently by __ __ and __ __. | Dmitri Mendeleev and Lothar Meyer
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| As you list elements on the periodic table in order of atomic mass, there is a distinct regular __ in their properties. | variation
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| The physical and chemical properties of the elements are periodic functions of their atomic numbers. This is called __ __. | periodic law
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| Metalloids (as listed on the periodic table) and like metals AND __. They are intermediate substances. | nonmetals
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| On the periodic table, a horizontal row of elements is called a __. | period
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| On the periodic table, a vertical column of elements is called a __. | group
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| Elements in a particular __, or family on the periodic table, share many similarities. | group
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| If a group on the periodic table has an A in front of it, that means the column features __ __. | main-group elements
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| If a group on the periodic table has an B in front of it, that means the column features __ __. | transitional elements
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| Elements that tend to lose electrons during chemical change are called __. They form positive ions. | metals
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| A substance whose atoms tend to gain electrons during chemical change are called __. They form negative ions. | nonmetals
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| Metals are found primarily in the left __ of the periodic table. | 2/3
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| Metals have high __ and __ conductivity. | electrical and thermal
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| Metals have high __ and __. | malleability and ductility (meaning they can be formed into thin wire)
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| Metals have a high __. | metallic luster
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| Most metals are __ at room temperature. | solid
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| Mercury, though a metal, is a __ at room temperature. | liquid
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| Nonmetals tend to gain __, forming negative ions. | electrons
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| Nonmetals can be found in the right __ of the periodic table. | 1/3
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| Nonmetals tend to be __. | brittle
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| Nonmetals are __ solids or gases. | powdery
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| Basically, nonmetal properties are the __ of metal properties. | opposite
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| Most periodic tables give the element __, atomic __, and atomic __. | symbol, atomic number, atomic mass
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| The primary factor in understanding how atoms join together to form compounds it the __ __. | electron arrangement
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| The arrangement of electrons in atoms is atom's __ __. | electron arrangement
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| The outermost electrons in an atom, which are involved in chemical bonding, are called __ __. | valence electrons
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| Bohr's model of the hydrogen atom didn't clearly explain the electron __ __ __ __. | structure of other atoms
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| Wave properties of electrons conflict finding their specific __. | location
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| Who developed the equations that took into account the particle nature and the wave nature of electrons? | Shroedinger
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| Schroedinger's equations allow us to determine the __ of finding an electron on a specific region of space. | probability
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| Each possible energy level of an electron has one or more __ or __. | sublevels or subshells
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| Each electronic sublevel contains one or more atomic __. | orbitals (remember, orbitals differ from orbits)
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| The first 4 sublevels are designated __. | s, p, d, f
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| The higher the energy level, the __ the electron is from the atomic nucleus. | farther
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| If an electron's principle energy level is 1, then it's sublevel is __ __. | also 1
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| The electron capacity of a principle energy level is __. | 2(n)^2
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| When determining how many electrons can in in a sublevel, you always __ the number of the sublevel. | double
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| A set of energy-equal orbitals within a principle energy level is called a __. | sublevel
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| Electrons in the 3d subshell have __ energy than electrons in the 3p subshell. | more
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| When describing the location of an atom, you must specify both the __ __ __ and the __. | principle energy level and the subshell
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| A specific region of a sublevel containing a maximum of 2 electrons is called an __. | orbital
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| Orbitals are named by their __ and their __ __ __. | sublevel and their principle energy level
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| Each type of orbital has a characteristic __. | shape
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| The S type orbital is __ symmetrical. | spherically
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| The P type orbital has a shape like a __. | dumbbell
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| The s subshell has _ orbital, and a maximum of __ electrons. | 1 orbital, 2 electrons
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| The p subshell has __ orbitals, and a maximum of __ electrons. | 3 orbitals, 6 electrons
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| The d subshell has __ orbitals, and a max of __ electrons. | 5 orbitals, 10 electrons
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| The f subshell has __ orbitals, and a max of __ electrons. | 7 orbitals, 14 electrons
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| The arrangement of electrons in atomic orbitals is called an __ __. | electronic configuration
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| The building up principle helps determine the electron configuration. Another phrase for the "building up" principle is the __ __. | Aufbau Principle
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| Electrons fill the __-__ orbital that is available first. | lowest-energy
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| Each orbital can hold up to 2 electrons with their spins in opposite directions. This is called the __ __ __. | Pauli Exclusions Principle
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| Each orbital in a subshell is half-filled with one electron and prior to filling the orbitals with 2 electrons. This describes __ __. | Hund's Rule
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| To write an electron's configuration, you must obtain the total number of __ in the atom from the atomic number. | electrons
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| To write an electron's configuration, you must remember that electrons occupy the __ energy orbitals that are available. That means __ comes first. | lowers, 1s
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| To write an electron's configuration, you must remember that each __ __ __ contains the same number of sublevels. | principle energy level
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| To write an electron's configuration, you must remember that the s sublevel has __ orbital, the p sublevel has __ orbitals, and the d sublevel has __ orbitals. | 1,3,5
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| To write an electron's configuration, you must remember that there can't be more than __ electrons in any orbital. | 2
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| To write an electron's configuration, you must fill orbitals from __ to __ energy. | lowest to highest
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| To write an electron's configuration, you must remember that the max number of electrons in any principal energy level is __. | 2(n)^2
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| Noble gases are extremely __. | stable
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| Noble gases are called __ because they don't readily bond to other elements. | inert
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| The stability of noble gases is due to a full complement of __ __ in the outermost s and p sublevels. | valence electrons
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| Elements usually react in such a way as to attain the electron configuration of the noble gas closest to them in the periodic table. This is called the __ __. | Octet Rule
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| Elements on the right side of the periodic table more right to the next __ __. | noble gas
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| Elements on the left side of the periodic table move __ to the noble gas of the previous row. | backward
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| Atoms will __, __, or __ electrons in chemical reactions to attain this more stable energy state. | gain, lose, or share
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| Elements in families (or groups) other than the noble gases are more __. | reactive
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| A stable electron configuration is called the __ __ configuration. | noble gas
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