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Metals
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Scientists
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Families
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Vocab
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Trends
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Grab Bag
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Metals Scientists Families Vocab Trends Grab Bag $100 $100 $100 $100 $100 $100 $200 $200 $200 $200 $200 $200 $300 $300 $300 $300 $300 $300 $400 $400 $400 $400 $400 $400 $500 $500 $500 $500 $500 $500
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Name 4 characteristics of metals.
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Shiny, malleable, ductile, and conductive
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Why do metals conduct electricity?
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Conductance is the ‘flow of electrons
Conductance is the ‘flow of electrons. Metals have a lower electronegativity, so they share their electrons with many neighboring atoms.
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Which type of bonds have delocalized electrons; metallic, covalent, and/or ionic?
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Metallic only. Covalent and ionic are localized around just two atoms.
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What does “sea of electrons” refer to in a metal?
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It’s the model of the electron structure of metals, where electrons are delocalized and free to move throughout the whole sample of atoms.
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What region of the periodic table do metals react with in order to become stable?
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The nonmetals
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Name the 3 scientists who contributed to the periodic table, in order.
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Newlands, Mendeleev, and Moseley
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Who arranged the periodic table by atomic number?
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Henry Moseley
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Who was the first scientist to arrange the periodic table by properties and the Law of Octaves?
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John Newlands
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Whose contribution was significant because he had better technology available to him?
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Henry Moseley
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Who left gaps in the periodic table?
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Dmitri Mendeleev
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Name the families on the periodic table in order from left to right & top to bottom.
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alkali metals, alkali-earth, transitions, halogens, noble gases, lanthanides, actinides
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Which family is radioactive?
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Actinides
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A bond made from a metal and a nonmetal is a _______bond.
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Ionic-metal/nonmetal. Covalent-two or more nonmetals
Ionic-metal/nonmetal *Covalent-two or more nonmetals *Metallic- all metals
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Which 2 families are the most reactive?
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Alkali metals and halogens
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Locate all of the transition metals on the periodic table.
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The d-block plus the lanthanides and actinides
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Define Octet Rule.
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The tendency of atoms to gain or lose electrons in order to become stable (refers mainly to filling the s and p orbitals.
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Define ionization energy.
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The energy required to remove an electron.
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Define electron affinity.
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The amount of energy released when an atom gains an electron.
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Define nuclear charge.
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The charge/strength of the protons in the nucleus.
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Explain reactivity.
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The ease in which atoms exchange electrons in order to become stable.
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Where on the periodic table is ionization energy the greatest?
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Top right.
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Which trend increases down a group but has no change across a period?
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The shielding effect. (electron shielding)
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Explain why atomic radius decreases across a period.
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The nuclear charge increases, and electrons are added to the same energy level, so the attraction is greater.
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Why does electron shielding increase down a group?
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Core electrons are added and the valence electrons are further from the nucleus.
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Daily Double!!
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Which atom has a lower ionization energy: silver (Ag), arsenic (As), or strontium (Sr)?
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Strontium, b/c it has more e- shielding than arsenic, and a greater desire to lose an e- than silver
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Which family tends to have a +2 charge?
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Alkaline-Earth Metals
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Why does group 16 have a -2 charge?
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Group 16 wants to gain 2 e- to fill it’s octet.
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Which family is slightly more dense, smaller, and less reactive than the alkali metals?
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Alkaline-earth metals
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Which family is slightly more dense and less reactive than the alkaline-earth metals?
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The transition metals
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Based on it’s e- configuration, why does helium have a high ionization energy?
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Because it’s already stable with it’s full s orbital, and would require a lot of energy to remove an e-
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Double Jeopardy!!
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Daily Double!!
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Write the Final Question Here
Jeopardy Write the Final Question Here
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Write the Final Answer Here
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