Q0-1:  Define the term PROTON.

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Q0-2:  Define the term NEUTRON.

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A0-2: A subatomic particle that has no charge and that is located in the nucleus of the atom.

Q0-3:  What is the ATOMIC NUMBER?

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Q0-4:  What is the MASS NUMBER?

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Q0-5:  What is an ISOTOPE?

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Q0-6:  How do you determine the number of neutrons in an atom?

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Q0-7:  What is Avogadro’s number?

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Q0-8:  What is a MOLE?

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A0-8:  One mole has been defined as the number of atoms in 12.00 grams of carbon-12 -- or, 6.022 x 10²³ particles of that substance.

Q0-9:  Determine the mass in grams of each of the following:    a) 2.5 mol of sulfur, S; b) 0.50 mol of carbon, C; c) 1.8 mol of calcium, Ca; d) 3.2 mol of copper, Cu

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Q2-1: What is the property used to organize elements in the modern periodic table?

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Q1-2: . Each row of the periodic table is called a ……….

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Q1-3: Each column of the periodic table is called a ………..

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Q1-4: Each rectangle on the periodic table represents one element. Inside the box are four pieces of information. State what these items mean. a) Top number: b) A letter(s) of the alphabet: c) A word: d) Bottom number:

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Q1-5: Who was the first chemist to design a way of organizing chemical elements?  
When did he publish the first periodic table?

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Q1-6: What pattern of organization did he use to arrange the elements?

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Q1-7: How are elements arranged in the modern periodic table?

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Q1-8: State the PERIODIC LAW:

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Q2-1: Why do elements within a group of the periodic table have similar chemical properties?

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A2-1: They have the same number of valence electrons and so react in similar ways to other elements.

Q2-2: What happens to an atom that gains or loses electrons?

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A2-2: These elements form positive or negative ions. Group 1 (alkali metals) loose an electron and become positive ions. Group 17 (halogens) gain an electron and become negative ions.

Q2-3: List the three main categories of elements and give an example of each.

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A2-3: metal - gold; non-metal - sulfur; semiconductor - silicon

Q2-4: What is a VALENCE ELECTRON?

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A2-4: Electrons in the outer energy level of an atom

Q2-5: What is an ION?

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A2-5: An atom, radical, or molecule that has gained or lost one or more electons and has a negative or positive charge.

Q2-6: Which periodic table group forms positive ions?

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A2-6:  Alkali metals (group 1)

Q2-7: Which periodic table group forms negative ions?

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A2-7: Halogens (group 17)

Q2-8: State the definition for a METAL.

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A2-8: An element that is shiny and conducts heat and electricity well.

Q2-9: State the definition for a NONMETAL.

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A2-9:  An element that conducts heat and electricity poorly.

Q2-10: State the definition for a SEMICONDUCTOR.

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A2-10:  An element or compound that conducts electric current better than an insulator does but not as well as a conductor does.

Q2-11: Which elements are DUCTILE and MALLEABLE?

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A2-11:   transition metals (ductile means it can be drawn out into wires -- like copper; malleable means it can be formed into shapes -- like silver or gold)

Q2-12: Explain why elements in a group on the periodic table have similar chemical properties.

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A2-12:  The chemical properties of each group are related to the number of valence electrons.

Q2-13:  Draw electron shell diagrams for the following elements:
a) Lithium     b) Sodium
c) Carbon      d) Oxygen

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A2-13: a) Li -- 2)1; b) Na --2)8)1; c) C -- 2)4; O -- 2)6

Q2-13: . Draw electron shell diagrams for the following elements:   e)Fluorine    
f) Neon   g)silicon       h) Argon

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A2-13: e) F -- 2)7; f) Ne -- 2)8; g) Si -- 2)8)4; h) Ar -- 2)8)8

Q3-1: What are the families of metals?

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A3-1: alkali metals, alkaline-earth metals, transition metals

Q3-2: What are two families of nonmetals?

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A3-2: halogens & noble gases

Q3-3: List 4 unusual facts about HYDROGEN.  

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A3-3: a) most abundant element in universe; b) 3 out of 4 atoms in the universe are hydrogen; c) with its one electron it can react with many other elements; d) it has just one proton and one electron

Q3-4: What is the name of Group 1 on the periodic table? ____________ .
Give two characteristics of that family. 

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A3-4: Alkali metals: a) highly reactive; b) have one valence electron; c) react with halogens to make salts; d) not found in pure form in nature; e) often stored in oil to prevent them from reacting with moisture in the air.

Q3-5: What is the name of Group 2 on the periodic table? Give 4 characteristics that are different from those of Group 1.

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A3-5: Alkaline-earth metals: a) have two valence electrons; b-e) are harder, denser, stronger, and have higher melting points than alkali metals

Q3-6: Name 3 transition metals used in making jewelry.  

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A3-6: gold, silver, platinum

Q3-7: Your classmate offers to give you a piece of sodium that he found on a hiking trip. What is your response? Explain.

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A3-7: The classmate did NOT find sodium because it is not found in its pure form in nature since it has one valence electron and reacts easily with other elements to form compounds like SALT.... NaCl

Q3-8: Which elements are synthetic?

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A3-8: All elements with an atomic number greater than 92 are synthetic.

Q3-9: What is unique about the valence numbers of elements in the family of Noble Gases?

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A3-9: Elements in the family of noble gases have a FULL outer shell of electrons -- either 2 (as in helium) or 8 (neon, argon, krypton, xenon, radon)

Q3-10: Why are atoms of Chlorine and Bromine very reactive?

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A3-10:  They have 7 valence electrons and need only one more electron to make a new compound. They react quickly with alkali metals to produce salts.

Q3-11: Classify the following elements as alkali, alkaline-earth, or transition metals based on their positions in the periodic table:     a) Fe    b) Sr     c) K      d) Pt

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A3-11: a) Fe -- transition metal; b) Sr -- alkaline-earth metal; c) K -- alkali metal; d) Pt -- transition metal

Q3-12: Draw valence diagrams for the following elements:  a) Li         b)B     

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Q3-12: Draw valence diagrams for the following elements:  c) N          d) F    

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Q3-12: Draw valence diagrams for the following elements:  e) Be         f) C   

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Q3-12: Draw valence diagrams for the following elements:  g) O         h) Ne

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Q4-1: How did Mendeleev arrange elements in the periodic table?

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A4-1:  by atomic mass

Q4-2: On what basis is the modern periodic table arranged?

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A4-2:  by atomic number

Q4-3: How can an element become an ion?

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A4-3:  by gaining or loosing one or more electrons

Q4-4: What are the three ways that elements can be classified?

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A4-4:  as a metal, non-metal, or semiconductor

Q4-5: What are the two things that each periodic table family have in common?

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A4-5: valence number and chemical properties

Q4-6: What are three metal families in the periodic table?

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A4-6:  alkali metal, alkaline-earth metal, transition metal

Q4-7: Name two families of nonmetals.

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A4-7:  halogens, noble gases

Q4-8: What is a semiconductor?

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A4-8:  An element that conducts heat and electricity better than an insulator but not as well as a conductor

Q4-9: What does an element’s atomic number represent?

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A4-9:  the number of protons (and electrons)

Q4-10: How do you determine the number of neutrons of an element?

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A4-10:  subtract the atomic number from the atomic mass

Q4-11: What is a valence electron?

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A4-11:  an electron(s) in the outer most shell (highest energy level) of an atom