Unit 3 Periodic
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| Who was the first person to mostly create the Periodic Table? | Dimitri Medeellev
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| Who was the first person to attempt to organize and predict gaps in the Periodic Table? | Newlands
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| What is the definition of "periodic"? | Occurring in a regular, repeating pattern
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| What did Mosely do? | Discovered each element contins a unique number of protons in a nucleus. He also rearranged Mendeleevs Periodic Table by number of protons/atomic number, rather than mass.
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| What is the Periodic Law? | When elements are changed by atomic number their chemical and physical properties show regular patterns of variation.
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| Which type of element is unreactive, has a full outermost energy level and has no bonding? | Noble Gases
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| What determines physical properties of an element and is arranged in families in the Periodic Table? | Having the same number of valence electrons.
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| The S + P orbitals is the __ group? | A or 'Representative Group'
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| The B + D orbitals is the __ group? | B
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| Which type of element tend to be... -good conductors -malleable -ductile -lustorus -solids at room temp | Metals
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| Which type of metals tends to be... -Good insulators -brittle -dull -often liquids and gases at room tepmperature | Non-metals
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| Which group is referred as the Alkai metals? | Group 1 or 1A
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| Which group is very reactive and explosive in water, has one valence electron, and never found pure in nature? | Group 1 or 1A
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| Which group is referred to as the Alkaline Earth Metals? | Group 2 or 2A
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| Which group is referred to as the Halogens? | Group 17 or 7A
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| Which group is... -generally non-reactive -has full/complete valence shell -8 valence electrons | Group 18 or Noble Gases
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| What is Atomic Radius? | The size of an atom.
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| What is Metallic Character? | The characteristic of an element that relates to metals.
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| What is Ionization Energy? | The amount of energy it takes to remove the highest energy electron from an atom (to create a +1 charge)
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| What is Electonegativity? | The ability of an element's atom to attract electrons
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| From bottom left to top right of the periodic table, which trends increase? | Atomic Radius and Metallic Character
(RACK EM! R-A-C-M is going down.)
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| From top right to bottom left of the periodic table, which trends decrease? | Atomic Radius and Metallic Character
(RACK RACK RACK-EM! R-A-C-M is going down.)
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| What are ions? | Charged particles that can be negative or positive.
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| Metals form what type of ions? | Cations
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| Nonmetals form what type of ions? | Anions
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| ______ (Positive or Negative) ions are smaller. | Positive +
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| ______ (Positive or Negative) ions are larger. | Negative -
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| What do ions form to obtain? | An octect. (Full outermost energy level of 8 valence electrons.)
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| A nuetral atom's Atomic # is equal _______ # which is also equal to Electron #. | Proton
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| Why do atoms lose valence electrons? | To form ions and/or get a full outermost energy level.
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| Why are fewer energy levels used when making ions? | Ions take electrons to make an even outermost energy so it's spread across less energy levels which makes it a smaller element.
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| Non-metals tend to ____ (gain or lose) electrons. Why? | Gain
They are less likely to use ionization energy; they want to to fill their outermost energy level.
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| Metals tend to _____ (gain or lose) electrons? Why? | Lose
Because they are more likely to use ionization energy because they want to give up electrons to have equal outermost energy levels.
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| What is Successive Ionization Energy? | Energy that takes from levels beyond the outermost level of valence electrons.
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| If an element has a high metallic character, it is ______ (unwilling/willing) to give up electrons. | Willing.
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| What is shielding? | When an atom is trying to pull in an electron but because of many electrons already in the way (due to energy levels/periods) it can not put it tight.
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| What is isoelectric? | When ions electrons equal to a nuetral atom and they are alike.
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