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95 Cards in this Set
- Front
- Back
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_________ proposed that the properties of the elements vary in a periodic manner with the atomic weight of the elements.
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Dimitri Mendeleev
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Mendeleev grouped elements with similar properties in (rows/ columns / groups of eight).
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columns
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In 1914 _________ found that the frequency of vibration of the X-rays emitted by each element when bombarded with cathode rays bore a simple relationship to the atomic numbers.
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Henry Mosely
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Complete the following: The periodic law specifies ...
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The periodic law specifies the chemical properties of the elements are periodic functions of their atomic numbers.
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What determines the energy level of an electron?
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The distance of the electron from the proton-containing nucleus.
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(T/F) The more energetic electrons orbit closest to the nucleus.
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F
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Who developed the "planetary model" of the atom?
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Niels Bohr
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(T/F) Seven is the maximal number of electron layers that any atom can contain.
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T
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(T/F) Each of the energy levels has a limit on the number of electrons it can hold.
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T
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How many electrons can the third energy level hold?
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18
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What equation specifies the maximum number of electrons an energy level can hold?
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2n₂
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What is the octet rule?
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The maximum number of electrons in the outermost energy level is 8.
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What is the electron configuration?
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The number and position of electrons in the energy levels of an atom.
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What is the electron configuration of the atom with an atomic number equal to 8?
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n1 = 2
n2 = 6 |
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What is the electron configuration of the atom with an atomic number equal to 16?
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n1 = 2
n2 = 8 n3 = 6 |
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What is the electron configuration of the atom with an atomic number equal to 20?
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n1 = 2
n2 = 8 n3 = 8 n4 = 2 |
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The electrons in the outermost energy level are called ...
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valence electrons
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What about the valence electrons is so important to the field of chemistry?
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The ability of the atom to gain or lose the valence electrons is what determines its chemical properties. Most chemical reactions involve the valence electrons; electrons in the inner layers are not important in normal circumstances.
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Elements in the periodic table are arranged in what two ways?
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Horizontally in rows in the order of increasing atomic number; vertically in columns according to their chemical properties.
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(T/F) All elements in vertical columns have the same number of valence electrons.
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T
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(T/F) Rows in the periodic table are called families or groups.
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F
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The alkali metals are located in what group number?
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1 or 1A
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The halogens are located in what group number?
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17 or 7A
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The noble gases are located in what group number?
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18 or 8A
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The alkaline earth metals are located in what group number?
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2 or 2A
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(T/F) Chemical properties change across rows, that is as you move from left to right within a period.
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T
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(T/F) With reference to the electronic configuration a new layer is added for each row or period in the periodic table.
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T
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(T/F) The energy level of the valence electrons is determined by the period it is in.
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T
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(T/F) The shape of the periodic table tells us where all of the electrons are in an atom.
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T
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(T/F) The maximal number of electrons in energy level 7 is 98.
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T
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Locate aluminum in the periodic table. How many valence electrons is there in a neutral atom of aluminum?
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3 valence electrons
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What is the dominant chemical property of the alkali metals group?
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They easily lose their single valence electron. Thus they are highly chemically reactive, especially with nonmetals.
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What are the two most common valences for the "transition elements?"
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1 and 2
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(T/F) The alkali metals exist in nature as diatomic molecules.
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F
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Why are the halogens so extremely reactive chemically?
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They seek an electron to complete their outermost electron level. We say they are highly electronegative.
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List the three classes of elements and designate their relative positions in the periodic table.
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metals are on the left side
nonmetals are on the extreme right side metalloids are in between |
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List four properties of metals.
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1. Conductors of heat and electricity
2. Will lose electrons when reacting with nonmetals 3. lustrous, malleable, and ductile 4. have high tensile strength (5). All are solids at room temperature except for mercury |
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Most metals are hard, strong and dense. Provide two examples of metals that are exceptions to this.
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Sodium (Na) is soft - you can cut it with a knife.
Mercury (Hg) is a liquid |
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(T/F) Metals belong to the families of elements with few electrons (1, 2, 3) in the outer energy level.
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T
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(T/F) Metals do not hold their valence electrons strongly and give them up easily.
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T
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(T/F) If not for their "loose" electrons, metals would not have their silvery luster, be malleable and ductile, or conduct electricity.
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T
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List four distinguishing properties of nonmetals.
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1. Poor cunductors of heat and electricity
2. tend to be brittle 3.examples of all physical states are observed at room temperature 4. many exist as diatomic molecules (5). they will gain electrons when reacting with metals, but share electrons when reacting with other nonmetals |
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Why do the halogens exist as diatomic molecules
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The sharing of an electron pair fulfils the outermost octet and stabilizes their chemical reactivity.
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Nonmetals may have from _____ to _____ valence electrons.
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4 to 8
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Which on of the following is not a nonmetal? (carbon / phosphorus / calcium / sulfur)
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calcium
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List three properties of metalloids.
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1. They have properties of both metals and nonmetals
2. They are more brittle than metals and less brittle than most nonmetaillic solids 3. They are semiconductors of electricity (4). They can act like metals when they react with nonmetals (5). They act like nonmetals when they react with metals |
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Which of the following is a metalloid? (S / Si / He / Fe).
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Si (silicon
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Provide the name of each of the following elements in the "ten most abundant" list.
O, Si, Al, Fe, Ca, Na, K, Mg, Ti, H |
Oxygen
Silicon Aluminum Iron Calcium Sodium Potassium Magnesium Titanium Hydrogen |
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Name two elemetns to represent each of these groups: alkali metals; alkaline-earth metals; transition elements; halogens; noble gases
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Identify the element that occupies Group 4A and is in the 6th period.
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Lead (Pb)
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What energy levels are the valence electrons in an atom of silver.
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5th
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Of the three classes of elements, what class is uranium in? (metal / metalloid / nonmetal)
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metal
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Elements with only a few valence electrons, which are given up easily, likely will be classified as ...
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metals
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They heavy zigzag in the periodic table separates what two elemental classifications?
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The zigzag line separates metals from nonmetals
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What is the class name of these "dividing" elements?
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The elements adjacent to this line are called the metalloids.
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Each electron level is made up of sublevels. Name the four types of sublevels.
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s, p, d, f
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Specify the maximum number of electrons that each of the four types of sublevels can hold.
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s = 2
p = 6 d = 10 f = 14 |
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What sublevels would exist in an atom with the atomic number = 8?
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s and p
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What sublevels would exist in an atom with the atomic number = 3?
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s and p
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What sublevels would exist in an atom with the atomic number = 18?
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s, p, and d
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Silicon is a major component of computer microchips because it is a (metal / nonmetal / metalloid / liquid)
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metalloid (semiconductor)
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What family has nine valence electrons?
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None, because the maximum number of valence electrons is eight.
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Elements in the same family have the same (atomic number / electron configuration / number of filled energy levels / number of valence electrons)
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number of valence electrons.
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Why do elements in the same family have similar properties?
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elements in the same family have similar properties because they have the same number of valence electrons.
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What is it about the atom that gives it metallic, nonmetallic, and metalloid properties?
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The valence electrons of metallic elements are held loosely and easily lost. Those of nonmetals are tightly held, and the nonmetal elements tend to gain electrons. Those of metalloids can be lost or retained, depending on external conditions.
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What makes Group 18 gasses "noble"?
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The outer shell of each noble gas atom contains eight electrons, so they are very stable and do not gain or lose electrons easily.
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Give two uses for the halogens and two uses for the noble gases.
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Cl₂as a disinfectant
F₂as a decay preventative Iodine prevents goiter or is a disinfectant He as a lifting gas Ne for illuminating signs Ar as an inert medium for welding |
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Name the electronic sublevels for levels 1 through 4.
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s, p, d, f
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Write the correct symbol of each of the named elements.
Hydrogen Sodium Iron Mercury Silicon Aluminum Helium Neon Argon Krypton Xenon Radon Gold Plutonium Carbon Potassium Copper Magnesium Oxygen Nitrogen Platinum Nickel Phosphorous Lithium Lead Silver Titanium Calcium Fluorine Chlorine Bromine Iodine Astatine Palladium Uranium Sulfur |
H
Na Fe Hg Si Al He Ne Ar Kr Xe Rn Au Pu C K Cu Mg O N Pt Ni P Li Pb Ag Ti Ca F Cl Br I At Pd U S |
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Group 1 elements that each have one valence electron
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Alkali metals
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Group 2 elements that each have 2 valence electrons.
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Alkaline-earth metals
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A homogeneous mixture of metals
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Alloy
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Capable of being drawn into wire.
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Ductile
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The number and position of electrons in the energy levels of an atom.
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Electron configuration
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The relative ability of an atom to attract electrons in a chemical bond.
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Electronegativity
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A vertical column in the Periodic Table. Also called a group.
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Family
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Another name for a "family" in the Periodic Table.
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Group
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Reactive elements in Group 7 that have seven valence electrons.
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Halogens
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Sheen, brightness, brilliance, or radiance of light.
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Luster
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Capable of being hammered or rolled
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Malleable
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Proposed that the properties of the elements vary in a periodic manner with the atomic weight of the elements.
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Dimitri Mendeleev
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A substance that tends to give up electrons in chemical reactions.
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Metals
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Found that the frequency of vibration of the X-rays emitted by each element when bombarded with cathode rays bore a simple relationship to the atomic numbers.
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Henry Moseley
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Stable elements found in group 8 that have eight valence electrons.
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Noble gases
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An element that tends to gain an electron in a chemical reaction; poor conductor of heat and electricity.
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Nonmetals
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Atoms are most stable if they have a filled or empty outer layer of electrons.
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Octet Rule
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A horizontal row in the Periodic Table; defines the total number of energy levels.
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Period
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The chemical properties of the elements are periodic functions of their atomic numbers.
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Periodic Law
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A table of elements arranged by atomic number into vertical columns called families or groups, and horizontal rows called periods.
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Periodic Table
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A substance that holds its electrons in a way that allows a partial flow of electricity.
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Semiconductor
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A period or row in the Periodic Table.
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Series
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Strong metals in Groups 1B-8B
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Transition elements
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An element with an atomic number higher than that of uranium.
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Transuranium elements
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The electrons in the outermost energy level.
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Valence electrons.
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What are the Diatomic elements?
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Hydrogen
Nitrogen Oxygen Fluorine Chlorine Bromine Iodine |
