Increasing electronegativity Use the figure provided to determine which of the following describes MgO. Select the correct answer below: nonpolar covalent ionic polar covalent none of the above
Which of the following describes how tightly an atom attracts electrons in a bond? Select the correct answer below: electronegativity ionization energy atomic radius electron affinity
Use the information below to answer the question that follows. N2(g) + 3H2(g) ⟶ 2NH3(g) Bond energy of (N≡N) = 941 kJ Bond energy of (H−H) = 436 kJ Bond energy of (N−H) = 391 kJ What is the enthalpy of the reaction using bond energies, in kilojoules? Round your answer to the nearest whole number. Provide your answer below: kJ
In general, when the absolute value of the difference in electronegativity of two bonded atoms is above 1.8, the bond is considered to be Select the correct answer below: pure covalent polar covalent ionic
After determining the total number of valence electrons, what is the next step that should be taken when drawing a Lewis structure? Select the correct answer below: Rearrange electrons of the outer atoms to make multiple bonds with the central atom. Draw a skeletal structure of the molecule or ion, arranging outer atoms symmetrically around a central atom. Place electrons on the central atom to fill its octet. Distribute the electrons as lone pairs on the outer atoms, completing an octet around each atom.
Which molecule will have a double bond? Select the correct answer below: CO CCl4 OF2 H2CO
What is the Lewis symbol for Be2+? Select the correct answer below: :Be2+ :Be2+ Be2+ :Be2+
The Lewis symbol for the chloride ion will have how many dots? Provide your answer below:
A Lewis symbol with no dots must be a: Select the correct answer below: cation anion neutral atom depends on the element
Which molecule will have a triple bond? Select the correct answer below: C2H2 C2H4 C2H6 C3H6
When drawing the Lewis structure for a molecule, after drawing the skeletal structure and distributing all of the electrons around the terminal atoms, what actions should be taken if the central atom does not have a complete octet? Select the correct answer below: Move a lone pair electrons from one or more outer atoms to the central atom. Rearrange lone pairs of electrons from the outer atom(s) to form double or triple bonds to the central atom. Rearrange lone pairs of electrons around the central atom to form double or triple bonds to an outer atom or atom(s). Add electrons to the central atom, and count how many were added so the charge of the molecule or ion can be adjusted.
What is the Lewis symbol for I−? Select the correct answer below: : I :- : I : : I ¨ : : I ˙ :
A Lewis symbol consisting of an S and 8 dots must be: Select the correct answer below: a neutral sulfur atom the sulfide anion a sulfur cation none of the above
Electrons on a Lewis symbol will be arranged: Select the correct answer below: in random order two on one side before filling another one on every side before placing a second on any side depends on the element
Which of the following is very reactive and can readily combine with molecules containing atoms with lone pairs? Select the correct answer below: hypervalent molecues odd-electron molecules electron-deficient molecules all of the above
The octet rule predicts that fluorine will tend to make bond(s). Select the correct answer below: 1 2 3 4
A phosphorus atom can make up to bonds in a Lewis structure. Provide your answer below:
We can predict the number of bonds an atom can form from: Select the correct answer below: the number of core electrons needed to form an octet the number of electrons needed to form an octet the size of the valence electrons all of the above