Chapter 11: Chemical Bonding
atoms of the metallic elements generally form ions by
c. losing electrons, forming positive ions
which type of chemical bond involves the equal sharing of electrons?
c. nonpolar covalent
elements of Group 6A generally form ions with a charge of
d. -2
what is the number of valence electrons in a chlorine atom in the ground state?
d. 7
what is the total number of valence electrons in a molecule of ammonia (a/n NH₃)?
d. 8
given the formula Sr₃P₂, what is the formula for barium and arsenic?
d. Ba₃As₂
which of the following 3rd period elements has the smallest atomic radius?
d. Cl (a/n bc it's smallest in the top right corner of PT)
which element forms an ion that is larger than its atom?
d. Nitrogen
a nonpolar covalent bond will form between which two atoms as shown in the following combinations?
d. chlorine and chlorine
the shape of a carbon tetrachloride CCl₄ molecule is
d. tetrehedral
the molecular shape shown in the following figure is
d. trigonal planar (a/n one in middle with three atoms connected by bars)
the shape of AsH₃ is
d. trigonal pyramid
a Lewis dot symbol shows
c. all the valence electrons in the ground state of an atom
alkaline earth metals generally form ions with a charge of
b. +2
what is the total number of electrons present in an O⁻² ion?
b. 10
what is the total number of valence electrons in a molecule of carbon dioxide?
b. 16
what is the total number of electrons present in a Ca⁺² ion?
b. 18
what is the total number of valence electrons in a lithium sulfide formula unit?
b. 8
which of the following is a nonpolar molecule?
b. CO₂
bonds between which of the following two elements would involve a complete transfer of electrons?
b. K and I (a/n it's ionic which is between a metal and a nonmetal)
given the formula Na₃P, what is the formula for lithium and nitrogen?
b. Li₃N
which one has a trigonal pyramidal (a/n dots) structure?
b. NH₃
which of the following molecules contain one lone pair of electrons on the central atom?
b. NH₃ (a/n ammonia)
which of the following elements have the largest atomic radius?
b. P
given the formula Cs₂O, what is the formula for rubidium and sulfur?
b. Rb₂S
which of the following atoms has the largest radius?
b. Te (a/n smallest in top right, biggest in bottom left)
an S²⁻ ion has an electron configuration similar to that of
b. argon
a Ca⁺² ion has an electron configuration similar to that of
b. argon (a/n bc it's after argon in atomic numbers on PT)
as one progresses from left to right across a period on the PT, atomic radius generally
b. decreases
atoms of the nonmetallic elements generally form ions by
b. gaining electrons, forming negative ions
a polar covalent bond will form between which two atoms as shown in the following combinations?
b. hydrogen and chlorine (a/n bc hydrogen is +1 charge and chlorine is -1 charge)
bond formed between elements with electronegativities 1.2 and 3.0 would be
b. non polar covalent
the shape of a boron trifluoride BF₃ molecule is
b. trigonal planar
halogens generally form ions with a charge of
c. -1
what is the total number of valence electrons present in a PO₄³⁻ ion?
c. 32
how many valence electrons are present in an atom of carbon in the ground state?
c. 4
in the following shape, the bond angles are
c. 90° (a/n atom in middle with four bars connecting to it)
which of the following would require the largest amount of energy to remove the second electron?
c. K
which of the following does not represent the correct formula for a compound of sodium?
c. NaS (a/n bc Na has a charge of 1+ and S has 2- so it isn't balanced)
which of the following ions has the largest radius?
c. O²⁻
which is not a linear molecule?
c. SO₂
which of the following does not have a noble gas electron configuration?
c. Sb⁺⁵
which of the following sets of atoms is arranged in order of increasing electronegativity?
c. Si, P, S (a/n lowest in lower left, highest in upper right)
which of the following series is ranked in order of increasing electronegativity?
c. Sr, Sn, N, O
which structure represents the best Lewis structure for O₂?
a. (a/n ....O=O.... // two dots on top, two on side)
alkali metals generally form ions with a charge of
a. +1
how many valence electrons are present in an atom of cesium in the ground state?
a. 1
how many valence electrons are present in an atom of hydrogen in the ground state?
a. 1
what is the total number of valence electrons present in a NO₂⁻ ion?
a. 18
what is the total number of valence electrons present in a NH₄⁺ ion?
a. 8
given the formula GaP, what is the formula for aluminum and nitrogen?
a. AlN
which of the following ions has the smallest radius?
a. Be²⁺
which of the following elements has the lowest ionization energy?
a. C
which of the following compounds contains a triple bond in its Lewis structure?
a. CO
given the formula BaS, what is the formula for calcium and oxygen?
a. CaO
in the PT, the elements having lowest ionization energy are present in
a. I group (a/n lowest on bottom left)
which of the following atoms has the largest radius?
a. Mg
as one progresses from top to bottom of a group on the PT, atomic radius generally
a. increases
which type of chemical bond involves the transfer of electrons?
a. ionic
which element forms an ion that is smaller than its atom?
a. lead