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Chem Only Review

3rd part of the final exam review for chemistry 1

QuestionAnswer
Elements in the same column have similar... outer level electron configurations
Outer level electron configurations change in a regular way from... one column to the next
As the principle quantum number (row number) increases, the size of the electron cloud... increases
How does the size of atoms develop as you look down the table? It increases
Why does the size of atoms decrease as you move across a period? One proton is added with each element, which means the electron cloud is pulled in tighter each time
How does the atomic radii of atoms increase within the periodic table? Top to bottom and right to left
In general, when atoms unite to form compounds... the compound is more stable than the uncombined atoms
Noble gas configurations are particularly stable because... the noble gases have filled outer energy levels
Chemists discuss the size of ions by referring to their... ionic radii
Metallic ions, on the left and in the center of the table, are formed by... the loss of electrons
Nonmetallic ions, located on the right side of the table, are formed by... the gain of electrons and are larger than the atoms from which they are formed
Metallic ions have an outer level that resembles that of... the noble gas at the end of the preceding period (the row above)
Non metallic ions have an outer level resembling that of... the noble gas at the end of the same period
The loss of one electron from the metals in Group 1 will give them the same configuration as... the noble gas at the end of the row above
What is the oxidation number(charge) of Group 1? 1+
What is the oxidation number(charge) of Group 2? 2+
What is the oxidation number(charge) of Group 13? 3+
What is the oxidation number(charge) of Group 14? 2+ or 4+
What is the oxidation number(charge) of Group 15? 3-
What is the oxidation number(charge) of Group 16? 2-
What is the oxidation number(charge) of Group 17? 1-
What is the oxidation number(charge) of Group 18? none, they don't normally form ions
What is ionization energy? The energy required to remove an electron from an atom
As you go down a column of the periodic table, ionization energy... decreases
What are two things that tend to lower ionization energy? Increased distance of the outer electrons from the nucleus and the shielding effect
What is the shielding effect? When inner electrons block the attraction of the nucleus for outer electrons
The number of electrons in the outermost sublevel is the same for all elements in a particular... group
Why does ionization energy increase as you move across a period? Because the nuclear charge increases
What is electron affinity? The attraction of an atom for an electron
The same factors that affect ionization energy also affect... electronegativity
As electronegativity increases, a(n) ____ in ionization energy can be expected. Increase
Metals have ___ electronegativities. Low
Nonmetals have ___ electronegativities. High
As you go down a group, the tendency to gain electrons _____. This is because atoms farther down the column are larger. (The nucleus is farther from the surface, and attracts the outer electrons ___ strongly.) Decreases, less
As you move across a period (left to right) what happens to the electronegativity? It increases
Are positive ions smaller or larger than the atoms from which they are produced? Smaller
Are negative ions smaller or larger than the atoms from which they are produced? Larger
Metals tend to ____ electrons. This means they have positive oxidation numbers. Lose
Nonmetals tend to ____ electrons. This means they have negative oxidation numbers. Gain
what is the electron configuration for Ne? [He] 2s2 2p6
what is the electron configuration for F? 1s2 2s2 2p5
what is the electron configuration for Si? 1s2 2s2 2p6 3s2 3p2
what is the electron configuration for K? 1s2 2s2 2p6 3s2 3p6 4s1
what is the electron configuration for Br? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
what is the electron configuration for Cu? 1s2 2s2 2p6 3s2 3p6 4s2 3d9
what is the noble-gas electron configuration for Sr? [Kr] 5s2
what is the noble-gas electron configuration for Ag? [Kr] 5s2 4d9
what is the electron configuration for sodium? 1s2 2s2 2p6 3s1
what is the electron configuration for Fe +2? 1s2 2s2 2p6 3s2 3p6 4s2 3d4
what is the electron configuration for bromine? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
what is the noble-gas electron configuration for barium? [Xe] 6s2
what is the noble-gas electron configuration for neptunium? [Rn] 5f4 6d1 7s2
what is the noble-gas electron configuration for cobalt? [Ar]4s2 3d7
what is the noble-gas electron configuration for silver? [Kr]5s2 4d9
what is the noble-gas electron configuration for tellurium? [Kr]5s2 4d10 5p4
what is the noble-gas electron configuration for radium? [Rn]7s2
what is the noble-gas electron configuration for lawrencium? [Rn]7s2 5f14 6d1
This electron configuration is for which element? 1s2 2s2 2p6 3s2 3p4 sulfur
This electron configuration is for which element?1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 rubidium
This electron configuration is for which element? [Kr]5s2 4d10 5p3 antimony
This electron configuration is for which element? [Xe]6s2 4f14 5d6 osmium
This electron configuration is for which element? [Rn]7s2 5f11 einsteinium
Created by: scwitty
 

 



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