WorksheetsEntrance Exam_Chem_Atomic Structure and Chemical Bonds
Total questions: 25
Worksheet time: 26mins
Based on the information in the table, which of the following arranges the bonds in order of decreasing polarity?
Cl–F > H–I > Se–N
Se–N > H–I > Cl–F
Cl–F > Se–N > H–I
H–I > Se–N > Cl–F
Which of the following correctly shows the bond polarity?
Which of the following best predicts the type of bond that forms between Br and Br?
Polar covalent
Nonpolar covalent
Ionic
Metallic
Which of the following bonds is likely to have the most ionic character?
Ca–S
P–Cl
Si–S
K–Cl
Which of the following bonds is likely to have the most ionic character?
N–F
Na–F
Mg–O
C–O
Which of the following best predicts the type of bond that forms between Cs and Cl?
Nonpolar covalent
Polar covalent
Ionic
Metallic
Which of the following correctly shows the bond polarity?
In which of the following ionic compounds is the force of attraction between cation and anion the strongest?
RbI
CsI
MgO
SrS
The energy required to separate the ions in a CsF crystal lattice into individual Cs+(g) and F-(g) ions is known as the lattice energy of CsF(s). As shown in the table below, the lattice energy of CsF(s) is smaller than the lattice energy of a similar compound, KF(s).
Which of the following best explains why the lattice energy of CsF is smaller than the lattice energy of KF?
Cs+ has a larger ionic radius than K+, so the distance between cation and anion is greater in CsF than in KF.
Cesium has a smaller first ionization energy than potassium, so less energy is required to form the Cs+ ion than to form the K+ ion.
Cesium and fluorine have a greater electronegativity difference than potassium and fluorine, so the Cs–F bond is more polar than the K–F bond.
Cs+ contains more core electrons than K+, so the valence electrons in Cs+ are more shielded from the nucleus than the valence electrons in K+.
The Lewis structure of I2 is shown below.
Which of the following compounds has a Lewis structure that is electronically identical to that of I2?
HCl
CO
N2
BrF
In the Lewis diagram below, E represents an unknown element.
Which of the following could be the identity of element E?
Si
P
S
Cl
Which of the following Lewis diagrams correctly shows the electronic structure of XeF3+?
Ethylamine, C2H7N, is a colorless gas with a strong odor similar to ammonia. The compound is commonly used in the manufacture of other chemicals, including certain dyes, herbicides, and pharmaceuticals. The skeletal structure of ethylamine is shown below.
Which of the following correctly completes the Lewis diagram of ethylamine?
The ground-state electron configuration for an element contains an unpaired 3s electron.
Which of the following is the identity of the element?
Li
Na
Mg
K
The ground-state electron configuration for an element is [Kr]4d15s2
You may also see this electron configuration written as [Kr]5s24d1
Which of the following is the identity of the element?
Sc
Kr
Sr
Y
Which of the following is the electron configuration for a K+ ion in the ground state?
Which of the following is the electron configuration for the valence electrons of Bi in the ground state?
Which of the following electron configurations represents the element with the highest electronegativity?
1s22s22p2
1s22s22p4
1s22s22p63s2
1s22s22p63s23p2
Consider the following ions: Cl-, K+, S2-, Ca2+
Which of the following best predicts the trend in radii for these ions?
S2- < Cl- < K+ < Ca2+
Cl- < S2- < Ca2+ < K+
K+ < Ca2+ < S2- < Cl-
Ca2+ < K+ < Cl- < S2-
The first five ionization energies for elements X and Y are shown below. The units are in kJ/mol.
Based on the data in the table, which of the following correctly identifies elements X and Y, respectively?
B and Al
Al and B
N and P
P and N
Based on periodic trends and the data in the table above, which of the following is the most probable value for the ionic radius of Al3+?
16 pm
51 pm
95 pm
172 pm
Which of the following correctly identifies the element with the higher first ionization energy, P or As, and provides the best justification?
P, because of its half filled p subshell
P, because of its smaller atomic radius
As, because of its greater nuclear charge
As, because of its larger valence orbitals
Which of the following ground-state electron configurations represents the element with the lowest electronegativity?
[Ar]3d104s24p4
[Ar]3d104s24p5
[Kr]4d25s2
[Kr]4d105s25p4
Which of the following is the most likely empirical formula of the ionic compound that forms between Ga and O?
GaO
Ga2O
Ga2O3
Ga2O5
The electron configurations of four different elements are shown below.
Element 1: 1s22s22p4
Element 2: [Ne]3s23p5
Element 3: [Ar]4s2
Element 4: [Ar]3d104s24p1
Based on their electron configurations, which of the following two elements are most likely to form an ionic compound with the empirical formula XY2?
Element 1 and Element 3
Element 1 and Element 4
Element 2 and Element 3
Element 2 and Element 4
