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Chemistry Test Ch 6

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maddyynelss's version from 2016-10-11 02:27

Section 1

Question Answer
Who is credited with the modern periodic table?Newlands(octaves), Mendeleev(modern), Mosley(atomic number)
What are the properties of metals?Solid at room temp, shiny, good conductors of heat and electricity, ductile, malleable, able to lose electrons easily
What are the properties of nonmetals?'Opposite of Metals', brittle, not maleable or ductile, poor conductors of heat and electricity, able to gain electrons easily
What are the properties of metalloids?PARTIALLY conduct heat and electricity, 'Mix of Metals and Nonmetals"
Which group are the Noble Gases located in?Group 18
Which Group are the Transition Metals located in?Groups 3-12
What group are the Halogens located in?Group 17
What group are the Alkali Metals located in?Group 1
What group are the Alkaline Earth Metals located in?Group 2
How to identify the number of Valence Electrons in a groupThe Group #---there are similar properties down a group
memorize

Section 2

Question Answer
Describe the S-Block on the Periodic TableThe Alkali Metals and the Alkali Earth Metals(Groups 1 and 2)**also helium, a maximum of two electrons
Describe the P-block on the Periodic TableGroups 13, 14, 15, 16, 17, and 18(except helium), a maximum of six electrons
Describe the D-block on the Periodic TableGroups 3, 4, 5, 6, 7, 8, 9, 10, 11, 12(also known as transition metals), a maximum of ten electrons
Describe the F-block on the Periodic TableThe Lanthanides and Actinides, maximum of thirteen electrons
How are electron configurations relate to location on the periodic table?look at image for details
How to identify the number of energy levels by the placement on the periodic tablethe period number tells the number of energy levels
memorize

 

Question Answer
Compare the radius of an element to it's ionpositive ions have a smaller radius, and negative ions have a greater radius(more than a normal ion for both)
What is the characteristic that is the most important in determining an elements properties?The number of Valence Electrons it has--if they are in the same group, they will have the same properties
What is successive ionization energies?Each ionization energy gets bigger--there is an especially big jump after the removal of outer electrons
memorize

 

Question Answer
Draw the where the s-block is on a periodic tableit should be in groups 1 and 2(and helium)
Draw where the p-block is on a periodic tableit should be in groups 13, 14, 15, 16, 17, and 18(NOT HELIUM)
Draw where the d-block is on a periodic tableit should be in groups 3, 4, 5, 6, 7, 8, 9, 10, 11, and 12
Draw where the f-block is on a periodic tableit should be in the anthinoids and lathanoids
How do electron configurations relate to location on the periodic table?(draw diagram)should show labeling on diagram of last "set" in an electron configuration
memorize

Section 3

Question Answer
Atomic Radius trend across a perioddecreases due to increasing Nuclear charge, increasing number of protons
Atomic Radius trend down a groupincreases due to added energy level and/or added increased shielding
Nuclear Charge trend across a periodincreases because the size of the atom is smaller and there are more protons
Nuclear Charge trend down a groupdecreases because the valence electrons are farther away from the nucleus and greater shielding
Shielding Effect trend across a periodremains the same due to the number of energy levels staying the same
Shielding Effect trend down a groupincreases because of more energy levels
memorize

 

Question Answer
Ionization Energy trend across a periodincreases because the size of the atom is smaller and there are more protons
Ionization Energy trend down a groupdecreases because the valence electrons are farther away from the nucleus
Electronegativity trend across a periodincreases because there are more protons and a smaller radius
Electronegativity trend down a groupdecreases due to more shielding and larger electrons
Metallic Character trend across a periodincreases because the attraction between the valence electrons and the nucleus is weaker
Metallic Character trend down a groupincreases because the atomic size is increasing
memorize

 

Question Answer
Reactivity trend across a period (metals)decreases because the atom wants to give away electrons, and they have more electrons
Reactivity trend down a group(metals)increases due to higher reactivity and the fact that it is easier for electrons to be given or taken away
Ionic Radius trend across a periodthe more it loses, the smaller it gets
Ionic Radius trend down a groupincreases due to more energy levels
Reactivity trend across a period(nonmetals)increases as you go UP a group because the electronegativity is higher
Reactivity trend down a group(nonmetals)increases because the atom is getting close to filling its 's' and 'p' orbitals
memorize

Section 4

Question Answer
Ion:charged particle caused by the gain or loss of electrons
Anion:positive ion from the loss of electrons
Cation:negative ion from the gain of electrons
Anion(bigger or smaller)?the negative ion is always BIGGER than it's ion
Cation(bigger or smaller)?a positive ion is always SMALLER than it's ion
memorize

 

Question Answer
Explain the properties of elements given in their electron configurationsit explains what group it is in--the final two characters show what region it's in, the region shows it's properties
Describe the exceptions to the periodic trend in ionization energiesthe exceptions occur after group 5
memorize

Section 5