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148 Cards in this Set
- Front
- Back
How are elements ordered in the modern periodic table?
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According to increasing atomic number.
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Mendeleev noticed that certain similarities in the chemical properties of elements appeared at regular intervals when the elements were arranged in order of increasing _________.
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Atomic mass.
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What does the modern periodic table state?
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The physical and chemical properties of an element are functions of its atomic number.
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What did the discovery of the noble gases do?
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Changed Mendeleev's periodic table.
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How did the discovery of the noble gases change Mendeleev's periodic table?
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It added a new group.
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What is the most distinctive property of the noble gases?
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They're largely unreactive.
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If an isotope of fluorine has a mass number of 19 and an atomic number of 9. How many protons and neutrons are in this atom?
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9 Protons.
10 Neutrons. |
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An isotope contains 53 protons, 78 neutrons, and 54 electrons. What is the atomic number? Mass number?
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The atomic number is 53, and the mass number is 131.
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Is a period of the periodic table horizontally placed or vertically placed?
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Horizontally.
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Is a group/family of the periodic table horizontally placed or vertically placed?
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Vertically.
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What is atomic mass?
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The mass of the atom.
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What is atomic number?
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The number of protons in the nucleus of an atom.
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What did Mendeleev do that was so monumental?
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He arranged elements in order of various properties and created the first periodic table, published in 1869.
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Who created periodic law?
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Mendeleev.
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Who improved Mendeleev's law?
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Mosley.
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State the periodic law.
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The chemical and physical properties of elements are periodic functions of their atomic number.
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What happens when elements are arranged in order of increasing atomic number?
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Elements with similar properties appear at regular intervals.
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What is an arrangement of elements in order of atomic numbers so that elements with similar properties fall in the same column/group?
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The periodic table.
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Noble gases are ________. (Unreactive or Reactive.)
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unreactive
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Who discovered the noble gases?
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John William Strutt & Sir William Ramsey the first.
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What is periodicity?
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Similar trends between elements.
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Noble gases undergo few chemical reactions.
True or False? |
True.
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For each period, how many elements are in each?
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2 in Period 1.
8 in Period 2. 8 in Period 3. 18 in Period 4. 18 in Period 5. 32 in Period 6. 32 in Period 7. |
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For each period, in what order do the sublevels fill?
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1s in Period 1.
2s2p in Period 2. 3s3p in Period 3. 4s3d4p in Period 4. 5s4d5p in Period 5. 6s4f5d6p in Period 6. 7s5f6d7p in Period 7. |
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How do you find period from electron configuration?
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Take the highest number. (NOT exponent.)
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What determines which block an element is in?
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The highest letter it contains. (s,p,d,f)
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What are the two exceptions to "block theory"? Why?
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He & H because of differing properties.
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What are group one elements?
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Alkali metals.
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Alkali metals have a _______ appearance and are ______.
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silvery, soft
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Are s-block elements chemically reactive metals?
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Yes.
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Group two elements are ___________ metals.
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alkaline-earth
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Group two elements are ______, denser, & _________ than alkali metals.
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harder, stronger
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What do alkaline-earth metals contain?
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A pair of electrons in their outermost sublevel.
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What does each d sublevel consist of?
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5 orbitals with a maximum of 2 electrons each.
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Which block consists of transition metals?
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The d-block.
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Transition metals are metals with typical ______ properties, they are ____ conductors of electricity, and they have _____ luster.
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metallic, good, high.
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Transition metals are relatively _______. (Reactive/Unreactive.)
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unreactive
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The d-block contains groups _-__.
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3, 12
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The p-block contains groups __-__.
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13, 18
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The s-block contains groups _-_.
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1, 2
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p-block elements + s-block elements = _______ elements
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main group
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The total number of electrons in atoms of the p-block in the highest occupied level is equal to what?
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The group number minus ten.
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Elements in the p-block vary in ______.
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properties
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The right-hand end of the p-block contains all of the ______, except for H & He.
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nonmetals
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All six metalloids are in the _-block.
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p
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Which group are halogens a part of?
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Group 17.
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Halogens are the most reactive ________.
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nonmetals
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P-block elements are _______ than s-block elements, but _______ and _____ dense than d-block.
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harder, softer, less
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_______ is the exception to p-block rules, because it's reactive.
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Bismuth
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F-block elements are ________ and _______.
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lanthanides, actinides
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______ elements are wedged between groups 3 & 4 and periods 6 & 7 on the periodic table.
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F-block
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There are ___ f-block elements between La& Hf called _______.
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14, lanthanides
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Lanthanides are _______ and similar in _______ to alkaline earth metals.
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shiny, reactivity
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14 f-block elements between Ac & Rf called actinides, and they are _____.
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radioactive
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The first four actinides, Th-Np are _____ the rest are ________.
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natural, created in laboratories
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The size of an atom is defined by it's what?
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Orbital's edge.
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What is atomic radius?
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Half the distance between the nuclei of identical atoms that are bonded together.
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From left to right, atomic radii ______ on the periodic table
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decreases
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How is the trend of smaller atoms across a period caused?
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By the increasing positive charge of the nucleus.
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Name the noble gases in order.
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He, Ne, Ar, Kr, Xe, and Rn.
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As electrons add to s and p sublevels, they are gradually pulled closer to the higher charged nucleus, resulting in a _______ in atomic radii.
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decrease
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The atomic radii of main group elements normally ________ down a group.
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increases
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How can an electron be removed from an atom?
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If enough energy is supplied.
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A + energy ---> A+ + e-
Label this. |
A = symbol of any element.
A+ = ion or A with a positive charge. |
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What is an ion?
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An atom/group of bonded atoms that has a positive or negative charge.
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What kind of ion does Sodium form?
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Na+
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What is ionization?
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Any process that results in the formation of an ion.
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What is ionization energy? (IE)
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The energy required to remove one electron form a neutral atom of an element.
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Why are measurements of ionization energies made on isolated atoms in the gas phase?
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To avoid influences from nearby atoms.
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What are ionization energies measured in?
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kj/mole
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Ionization energies ________ with groups like H-Cs.
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decreases
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Group one metals have the ________ first ionization energies in their respective periods.
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lowest
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The higher the reactivity of a metal, the _______ electron loss is.
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easier
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Ionization energies of main group elements ________ across each period.
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increase
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Ionization energies of main group elements _______ across each period.
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increase
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Why do ionization energies of main group elements increase across each period?
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Because of the increasing nuclear charge.
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A ______ charge attracts electrons in the same energy level. (Ionization energies.)
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higher
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What is responsible for both increasing ionization energies and decreasing atomic radii across periods?
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Increasing nuclear charge.
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Generally, nonmetals have higher ___________ than metals.
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ionization energies
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Group 1 has the ______ ionization energy and an element of Group 18 has the _______.
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lowest, highest
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Among main group elements, ionization energies generally ______ down the groups.
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decrease
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As atomic number increases going down a group, _______ lie between the nucleus and the electrons in the highest occupied energy levels.
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electrons
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How can electrons can be removed from positive ions as well as from neutral atoms?
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Sufficient energy must be supplied.
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The energies for the removal of additional electrons from an atom are referred to as the what?
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Second ionization energy (IE2), third ionization energy (IE3), and so on. (*)
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The second ionization energy is always ____ than the first, third is _____ than second, etc.
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higher, higher
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Why do fewer electrons remain within the atom to shield the attractive force of the nucleus? (Ionization energies.)
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Because electrons are removed in successive ionizations.
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Each successive electron removed from an ion feels an increasingly _______ effective nuclear charge. (The nuclear charge minus the electron.)
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stronger
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Removing a single electron from an atom in of a group 18 element is ______ than removing an electron form atoms of other elements in the same period. (Harder or easier?)
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harder
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Can neutral atoms acquire electrons?
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Yes.
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What is called the atoms electron affinity?
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The energy change that occurs when an electron is acquired by a neutral atom.
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What do most atoms do when they acquire an electron?
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Release energy.
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Some atoms must be "forced" to gain an electron by the _____ of energy.
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addition
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Elements are more likely to form what kind of ions with lower ionization energies?
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Positive.
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Ions are very ______ making their electron affinity is very hard to determine.
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unstable
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Electron affinity is measured in ______.
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kJ/mole
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______ gain electrons the most often.
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Halogens
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Generally, as electrons add to the same p sublevel of atoms with increasing nuclear charge electron affinities become more ______ across each period within the p- block. (Groups 14-15 are exceptions.)
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negative
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Outer level electrons are what kind of electrons?
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Valence.
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Lanthinides and Actinides are in group 3.
True or False? |
False, they are groupless.
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Ca+ _____ an electron.
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removes
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Ca- ______ an electron.
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adds
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O2- adds _____ electron(s).
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2.
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Electrons typically _______ down a group in electron affinities.
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decrease
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A slight increase in effective nuclear charges down a group ______ electron affinities.
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increases
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An _______ in atomic radius down a group decreases electron affinities.
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increase
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Exceptions to group trends in electron affinities are _______________, which tend to be the same size or even decreasing down a group.
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heavy transition metals
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Certain p-block nonmetals tend to form _____ ions.
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negative
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Group 16 elements are present in many compounds as __ ions, (O, which sometimes achieves the configuration of Ne.)
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2-
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What is a positive ion called?
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A cation.
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The formation of a cation by the loss of 1+ electron always leads to what? Why? What happens to the remaining electrons?
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A decrease in atomic radius. Because of the removal of the highest energy level electrons results in a smaller electron cloud. They're drawn closer to the nucleus by its unbalanced negative charge.
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What is a negative ion called?
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An anion.
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How are anions formed?
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By the addition of one or more electrons.
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What does the formation of anions lead to?
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An increase in atomic radius.
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Why does the formation of anions lead to an increase in atomic radius?
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Because the total positive charge of the nucleus remains unchanged when an electron is added to the atom/ion therefore electrons are not drawn to the nucleus as strongly as they were before the addition of the extra electron.
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Why does the electron cloud spread out when anions are formed?
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Because of greater repulsion between the increasing number of electrons.
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Metals at the left end of the table form ______.
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cations
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Nonmetals at upper right tend to form ________.
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anions
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Do cationic radii decrease or increase across a period? Why?
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Decrease. Because the electron cloud shrinks due to increasing nuclear charge acting on the electrons in the same main energy level.
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Starting in Group __, anions are more common than cations.
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15.
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Why does anionic radii decrease across each period for the elements in Group 15-18?
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The same reason why carionic radii decrease from left-right across a period.
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Outer electrons in cations and anions are in ______ energy levels as one reads down a group.
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higher
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There is a gradual _______ of atomic radii down a group, there's also a gradual ______ of ionic radii.
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increase, increase
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Why do chemical compounds form?
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Because electrons are lost, gained, or shared between atoms.
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What are electrons that are available to be lost, gained, or shared in the formation of chemical compounds?
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Valence electrons.
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Where are valence electrons often located?
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In incompletely filled main energy levels.
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The electron lost between Na & Na+ is what kind?
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A valence electron!
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Main group elements' valence electrons are in the ________ s & p sublevels.
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outermost
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Respectively, Group 1 & 2 elements have ____ or ____ valence electrons.
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one, two
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Elements of Groups 13-18 have a number of valence electrons equal to what?
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The group number minus 10.
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Sometimes both s & p sublevel valence electrons of the p-block are involved in compound form.
True or False? |
True.
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Valence electrons hold atoms together in what?
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Chemical compounds.
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Who devised a scale of numerical values reflecting the tendency of an atom to attract electrons?
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Linus Pauling.
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What is electronegativity?
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A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.
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What is the most electronegative element? (4)
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Fluorine.
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Electronegatives tend to _______ across each period.
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increase
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Aklaki and alkaline-earth metals are the ______ electronegative elements.
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least
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Electronegatives tend to _______ down a group or remain about the same.
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decrease
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Why are the noble gases not assigned electronegativity?
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Because they do not form compounds.
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When a noble gas does form a compound, its electronegativity is extremely ____, similar to halogens.
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high
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Where are the elements with the highest electronegativity located on the periodic table?
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The upper-right.
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Where are elements with the lowest electronegativity located on the periodic table?
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The lower-left.
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D-block elements are all ______.
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metals.
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Ionization energies of the f-block and d-block elements generally _______ across the periods.
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increase
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The first ionization energies of the d-block elements generally ______ down each group.
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increase
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Why do the first ionization energies of the d-block elements generally increase down each group?
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Because the electrons available for ionization in the outer s sublevels are less shielded from the increasing nuclear charge by electrons in the incomplete (n-1)d sublevels.
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Among all the atoms of the d-block and f-block elements, electrons in the highest occupied sublevel are always removed ______.
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first
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Most d-block elements commonly form ____ ions in compounds
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2+
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Only the active metals of Groups __-__ have low electronegatives.
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1, 2
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