Unit 5 Chemistry Test – Flashcards
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Dmitri Mendeleev
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created periodic table and organized according to their properties
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Henry Mosey
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re-organized periodic table according to their atomic mass
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Which elements have an atomic radius greater than their ionic radius?
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metals which become cations
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Which element in Period 3 has the greatest tendency to gain electrons?
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Chlorine
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Which atom in group 17 has the strongest attraction for electrons?
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Fluorine
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Which atom in group 1 loses electrons most readily?
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Francium
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Elements that readily gain electrons tend to have high or low ionization energy and high or low electronegativity?
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high and high
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Electron Affinity
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energy change that occurs when an electron is acquired by a neutral atom
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Cation
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positive ion with smaller electron cloud and atomic radius
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Anion
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negative ion with larger electron cloud and atomic radius
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Electronegativity
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measure of ability of an atom in chemical compound to attract electrons
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Fluorine
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arbitrarily assigned an electronegativity of four
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Identify the most- an least- electronegative groups of elements in the periodic table
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Alkali Metals have the least electronegativity and the Halogens have the highest electronegativity
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Identify groups/families on the periodic table [left to right]
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Alkali Metals, Alkaline Earth Metals, Transitional Metals, Boron Family, Carbon Family, Nitrogen Family, Oxygen Family, Halogen Family, Noble Gas Family, Lanthanides, Actinides
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In order of the Periodic Table from left to right; metalloids, metals, non metals
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Metals, Nonmetals, Metalloids
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Periods
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horizontal rows on the periodic table
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Main group elements in the same family have?
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similar properties, same number of valence electrons, & (sometimes) the same oxidation number
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Reactivity does what, going down a metal and nonmetal group?
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reactivity increases down in a group of metals and decreases down in a group of nonmetals
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Identify main group elements
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s- and p-block also known as A groups
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Identify transition metals
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d-block also known as B groups
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Ionic Radius
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radius of an atom's ion
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Trends
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electronegativity, ionization energy, electron affinity, and atomic radius
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General trends for Atomic Radius [group and period]
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period: left to right - greatest to least
group: up to down - least to greatest
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Reasoning for the trends
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ionization energy: energy required to remove an electron,
electronegativity: tendency of an atom to attract electrons,
atomic radius: one-half the distance between the nuclei of identical atoms bonded together,
ionic radius: cations (decrease in radius), and anions (increase in radius)
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Cation radius to neutral ion
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positive ion is smaller bc when there's less electrons, the electromagnetic attraction is greater, meaning atomic radius is smaller
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Anion radius to neutral ion
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negative ion is larger bc when there's more electrons, the electromagnetic attraction is smaller, meaning atomic radius is larger
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General trends for electronegativity [group and period]
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period: left to right - least to greatest
group: up to down - greatest to least
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General trends for electron affinity [group and period]
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period: left to right - least to greatest
group: up to down - greatest to least
