Periodic Properties of the Elements (Ch7)
Why does atomic radius increase as you move right on the periodic table?
Effective nuclear charge increases, so core electrons are less able to shield outer electrons from nuclear charge and they are pulled closer.
Which has the higher lattice energy, NaCl or MgO?
Mgo
What are the bond angles of tetrahedral geometry?
109.5°
Which electron on xenon is the least shielded from the nuclear charge?
a. an electron in the 1s orbital
b. an electron in the 2s orbital
c. an electron in the 2p orbital
d. an electron in the 3p orbital
a. an electron in the 1s orbital
Which has the lower first ionization energy, Al or Mg? Why?
Aluminum has the lower first ionization energy because the electron is being removed from a higher energy p orbital.
What are the angles between hydrogen atoms in H3O+ ? Take O to be the central atom.
Slightly less than 109.5
Arrange the ions K+, Cl–, Ca2+, and S2– in order of increasing atomic radius.
Ca2+ < K+ < Cl– < S2–
What is the average formal charge of an oxygen atom in NO3–?
-2/3
What are the electron domain and molecular geometries for TeCl4?
Electron domain geometry: trigonal bipyramidal
Molecular geometry: seesaw
Arrange the atoms Ne, Na, P, Ar, K in order of increasing first ionization energy.
K < Na < P < Ar < Ne
From the options given below, choose the general valence electron configuration of elements that are most likely to form an ionic compound with an element with the ns2np5 general valence electron configuration.
a. ns2np6
b. ns2np5
c. ns2np4
d. ns2np2
e. ns2
e. ns2
Determine the hybridization of the central atom in NH4+.
Nitrogen is sp3 hybridized
Reactivity increases because ionization energy decreases, so it is easier to remove electrons.
On average, which has the shorter phosphrous-oxygen bonds, PO33– or PO43– ?
PO43– has the shorter average P-H bonds.
Which of the following species has bond angles that are slightly smaller than the ideal bond angles? Why?
PCl3, CCl4, SF6
PCl3 due to lone pair on central atom.