Basic Chem Test #2
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| What is the smallest particle of an element that retains the characteristics of that element? | Atom
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| A type of matter that has a fixed/definite composition: | Pure Matter
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| What are the 2 different categories of pure matter? | Elements and Compounds
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| The type of matter that is composed of only ONE type of atom. It cannot be broken down into simpler substances. | Element
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| Two or more substances that are physically mixed, but not chemically combined: | Mixture
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| This matter consists of a combination of 2 or more elements, always in the same ration: | Compound
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| This type of mixture is uniform throughout the sample (ex: air or salt water): | Homogenous
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| The components of this type of mixture do NOT have a uniform composition throughout the sample (ex: oil & water): | Heterogenous
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| Characteristics of an element that can be observed or measured without affecting the identity of the element: | Physical Properties
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| A foundation source of information concerning the known elements: | Periodic Table
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| This number on the periodic table physically IDENTIFIES the element. It also represents the number of PROTONS in one atom of that element: | Atomic Number
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| This is equal to the sum of the protons and neutrons in the nucleus of 1 atom of that specific element: | Mass Number
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| This number on the periodic table is relative to the element's weighted average of mass using an "average atom." | Atomic Mass
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| This is the decimal number below any given element on the periodic table: | Atomic Mass
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| This is the whole number located above any given element on the periodic table: | Atomic Number
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| The ______ and the _______ "live" in the nucleus of an atom. | protons and neutrons
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| The mass of an atom is contained in the ________. | nucleus
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| The nucleus of an atom has a _________ charge. | positive
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| Atoms of the same element that differ ONLY in mass (meaning, they differ in the # of neutrons): | Isotopes
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| In Isotopic Notation, that particular atom's _______ _______ is located to the upper left of the chemical symbol, while the _______ ________ of the element is located to the lower left. | Mass Number / Atomic Number
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| If an isotope of Flourine has a mass number of 19, and an atomic number of 9, it must have ___ neutrons present in the nucleus. | 10
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| In an atom, these are the chemically active electrons: | Valence Electrons
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| Group ___ ___ on the periodic table contains the chemically inert gases. | 8A
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| Each horizontal row of the periodic table is a: | Period
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| Each vertical column of the periodic table is a: | Group
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| "Families" of elements on the periodic table that have similar properties: | Groups
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| In Groups 1A-8A, the group number indicates the number of ________ __________ for the elements in each vertical column. | valence electrons
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| The physical arrangement of the elements in the MODERN periodic table is in order of increasing _______ ________. | atomic number
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| The ________ _______ states that the properties of elements recur in a repeating pattern when arranged according to increasing atomic number. | Periodic Law
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| Part of Dalton's Atomic Theory was that all atoms of a given element are identical in mass and properties. HOWEVER, the discovery the ________ by Chadwick in 1932 brought about the realization atoms in a given element can have different masses. | neutron
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| This subatomic particle has no electrical charge, but it DOES have a mass: | Neutron
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| This subatomic particle has great kinetic energy: | Electron
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| Generally, the energy levels closest to the nucleus contain electrons with the _________ energies, while the energy levels farther away contain electrons with ________ energies. | lower / higher
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| "A" Groups contain _________ elements. | Representative
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| "B" Groups contain __________ elements. | Transition
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| __________ elements are all metals. | Transition
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| __________ elements have variable valences, while ___________ elements have valences that correspond directly with their group number. | Transition / Representative
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| __________ elements have rather predictable reactions, whereas _________ elements are less predictable. | Representative / Transition
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| _________ electrons are the electrons in the outermost energy level of an atom. | Valence
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| An _______-____ symbol is a convenient way to represent the valence electron of an atom of an element. | Electron-dot
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| The distance from the atom's nucleus to the valence (outermost) electrons is the: | Atomic Radius
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| The larger the ________ ________, the larger the atom's volume | Atomic Radius
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| In Representative Elements (A Groups), the atomic radius _________ within a group from top to bottom, and _________ from left to right across a period | increases / decreases
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| Electrons are held in atoms by their attraction to the _________. | nucleus
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| The energy needed to remove the least tightly bound electron from an atom in the gaseous state: | Ionization Energy
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| When an electron is removed from a neutral atom, a particle called a __________ with a ________ charge is formed. | cation / positive
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| The ionization energy _______ within a group from top to bottom, but ________ from left to right across a period. | decreases / increases
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| Which element in the group 3A (on the periodic table) requires the most amount of energy to move 1 valence electron? | Boron (B)
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| Which specific cation will Al (aluminum) form? | Al 3+
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| How do metal atoms form ions? | They LOSE valence electrons, thus forming POSITIVE ions.
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| How do non-metals form ions? | They GAIN valence electrons, thus forming negative ions.
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| When a metal atom loses ALL of its valence electrons, it becomes a positive ion called a(n) ________. | cation
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| When a nonmetal atom gains enough valence electrons to form an octet (8 valence electrons), it becomes a negative ion called a(n) _______. | anion
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| What is the equation for Ionization Energy? | Na(g)+ energy (ionization) --> Na+(g) + e-
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| Mass Number is associated with which part of the atom? | The nucleus (because it is the SUM of the number of protons and number of neutrons, which both reside in the nucleus!
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| The radius of an atom will tell us its relative __________. | volume
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| The net charge of an atom is: | Zero (it's neutral)
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| The number of electrons in an atom is equal to the number of its _________. | protons
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| The average atom used to determine Atomic Mass is based on the mass of each isotope times the ________ ________. | percent abundance
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| What are the relative masses of the subatomic particles? | proton = 1 amu, neutron = 1 amu, electron = 0 amu
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| What is the symbol for a neutron? | n^0
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| What is the symbol for an electron? | e^-
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| What is the symbol for a proton? | p^-
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| What is a proton's electrical charge? | 1+
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| What is an electron's electrical charge? | 1-
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| What is a neutron's electrical charge? | 0
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| What is the unit used in measuring the mass of a subatomic particle? | amu (atomic mass unit)
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| Give the number of electrons, protons, and neutrons in one aton mof Oxygen-18: | The Atomic Number for Oxygen is 8, meaning it has 8 protons. 18 is the Mass Number for this specific atom of oxygen, which is the sum of the # of protons and the # of neutrons in the nucleus of the atom. Mass # - Atomic # = # of neutrons. (10 n^0)
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| What is the solid geometric form of an atom? | Sphere
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| Where are valence electrons located? | In the outermost energy levels
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| An atom has 5 electrons and 7 neutrons. This atom is an atom of which element? This atom is which specific atom? | It has 5 electrons, meaning it also has 5 protons. The element with the Atomic # of 5 on the Periodic Table is Boron (B). More specifically, this is an atom of Boron-12.
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| Write the electron energy levels arrangement for an atom of fluorine: | 1s^2 2s^2 2p^5
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| Which subatomic particle relates to the volume of an atom? | The electron (because its volume is determined by the atomic radius, which is created by the electron cloud)
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