Practice: Determine the bond angle of the following compound. AsCl_{5}

Subjects

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Molecular vs Electron Geometry | 27 mins | 0 completed | Learn |

Bond Angles | 10 mins | 0 completed | Learn Summary |

Hybridization | 26 mins | 0 completed | Learn |

Molecular Orbital Theory | 19 mins | 0 completed | Learn |

Heteronuclear Diatomic Molecules | 10 mins | 0 completed | Learn |

Additional Practice |
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Orbital Overlap |

Bond Order |

Delocalized Electrons |

Homonuclear Diatomic Molecules |

Additional Guides |
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Molecular Geometry |

VSEPR Theory |

Electronegativity |

According to the **VSEPR**** Model**, bond angles result from surrounding elements and lone pairs around the central element positioning themselves at an optimal distance.

Concept #1: VSEPR Model for Bonding

**Transcript**

Just realize according to the valence shell electron pair repulsion model or VSEPR model, we're going to say bond and lone pairs will position themselves around the central element so that they are as far apart as possible.

We said this before, if we have lone pairs, lone pairs are like pure energy. They want to push away all the bonds away from them. The bonds will position themselves as far away if possible from each other, but also as far away as possible from the lone pairs that exists around the central element. That's what the VSEPR model tries to explain. It's a way of describing what the molecular geometry is and why does it look the way that it does.

The **Valence Shell Electron Pair Repulsion **(VSEPR) theory gives bond angles based on the number of groups around the central element.

Concept #2: Ideal Bond Angles

**Transcript**

Based on the electronic geometry that we have, we have certain types of idealized bond angles, so ideal bond angles. So if your electronic geometry is AX2, your electronic region is two. AX3, AX4, AX5, AX6. That's what we mean by the electron regions. That just means how many groups are around my central element.

We know if you're AX2, then you're linear, so your ideal bond angle is 180 degrees. If your trigonal planer, it's 120. If you're tetrahedral, it's 109.5. If you're trigonal bipyramidal or you're trigonal bipyramidal, you have all of these angles involved. Then, if you're octahedral, you have 90 and 180.

The more lone pairs on the central element then the more compressed the bond angle, and the greater the deviation from an *ideal *bond angle.

Concept #3: Lone Pairs & Bond Angles

**Transcript**

What we should realize here is that those ideal bond angles aren't the same for every known compound. Here's the thing, we're going to say those ideal bond angles exist only if our central element has no lone pairs. Once our central element starts to get lone pairs, it's going to compress the bond angle. It's going to make it smaller.

Here we can see an example. Here we have methane which is CH4. Its electronic geometry will be AX4. It has no electron pairs around it, no lone pairs around the central element, so its ideal bond angle, its perfect bond angle would be 109.5.

But if we moved over to ammonia, NH3, we have our first lone pair involved. Lone pairs want to be as far away as everyone else. This is going to push the other bonds away from it. This causes them to compress or get smaller and that actually makes the bond angle smaller.

Water, now we have an additional bond angle, getting smaller, because now there are two lone pairs pushing away.

What you're supposed to take from this is those ideal bond angles are only if the central element has no lone pairs. Once the central element starts to have lone pairs the bond is going to get smaller and smaller.

Of course, your professor is not going to want you to memorize every single bond angle known to man. All you would have to say is, you don't need to know this exact bond angle, all you need to know is that the electronic geometry is AX4, so technically it's tetrahedral. The ideal bond angle is 109.5, but because that lone pair is there, all you'd have to really say is, you would expect the bond angle to be less than 109.5.

Here, since you have two lone pairs, you could say the same exact thing again, its electronic geometry is still AX4, ideally, it should be 109.5, but the lone pairs being there, make it less than 109.5.

This is what your professor would be looking for and this is what you would have to say.

Example #1: Determine the bond angles of each of the following compounds.

CO_{2}

Example #2: Determine the bond angles of each of the following compounds.

BrF_{4}^{+}

Practice: Determine the bond angle of the following compound. AsCl_{5}

Practice: Determine the bond angle of the following compound: IF_{3}.

0 of 7 completed

Concept #1: VSEPR Model for Bonding

Concept #2: Ideal Bond Angles

Concept #3: Lone Pairs Bond Angles

Example #1: Determine the bond angles of each of the followi...

Example #2: Determine the bond angles of each of the followi...

Practice #1: Determine the bond angle of the following compo...

Practice #2: Determine the bond angle of the following compo...

Which of the following molecules or ions has the smallest H-N-H bond angle?
NH4+
NH3
NH2−
H2N-NH2
H2N-CH3

The bond angles in NO2Cl (N is the central atom) are
1. 90°
2. < 190.5°
3. 109.5°
4. 120°
5. < 120°

Of the following, which molecule has the largest bond angle?
A. SO3
B. SF2
C. HCN
D. H2S
E. PF3

If PBr3Cl2 is a nonpolar molecule, determine the Cl—P—Br bond angle.
a. 120
b. 180
c. 90
d. 109
e. 55

If PBr3Cl2 is a nonpolar molecule, determine the Cl-P-Br bond angle?
a. 120
b. 180
c. 90
d. 109
e. 55

What is the value of the smallest bond angle in XeBr 4?
a. 109.5
b. 120
c. 90
d. 180
e. 45

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule.
SeO2 SeCl 6 SeF2
A) SeCl6 < SeF2 < SeO2
B) SeF2 < SeO2 < SeCl6
C) SeF2 < SeCl6 < SeO2
D) SeO2 < SeF2 < SeCl6
E) SeCl6 < SeO2 < SeF2

The C—N—O bond angle in nitromethane, CH3NO2, is expected to be approximately
1) 60°
2) 90°
3) 109.5°
4) 120°
5) 180°

Which molecule has the smallest bond angles?
a) CO2
b) H2O
c) NH3
d) BF3
e) CCl4

Which one of the following molecules and ions will definitely have at least one 90° bond angle in it?
(In each case except water, the central atom is the first one in the formula.)
a) AlCl4 -
b) NH3
c) PCl5
d) CO2
e) H2O

Draw the Lewis structure of BrF3 and determine the bond angle between an equatorial F atom and an axial F atom
= 90º
< 90º
> 120º
= 120
= 109.5º

Of the following molecules given below, which has the largest bond angle?
a) SO3
b) SF2
c) HCN
d) H2S
e) PF3

What is the actual bond angle between oxygen-sulfur bonds on molecules of SO 3?
(a) 109.5°
(b) < 109.5°
(c) > 109.5°
(d) 120°
(e) <120°

What set of species is arranged in order of increasing O–N–O bond angle?
a) NO2–, NO2, NO2+
b) NO2, NO2–, NO2+
c) NO2+, NO2, NO2–
d) NO2, NO2+, NO2–

Which has the largest bond angle?
a) angle O–S–O in SO42–
b) angle Cl–C–Cl in HCCl 3
c) angle in F–Be–F in BeF2
d) angle in H–O–H in H 2O

The O–Si–O bond angles in SiO2 (quartz) are closest to
a) 180°
b) 120°
c) 110°
d) 100°

The molecule below has been detected in gas clouds between stars. The predicted
C–N–H bond angle is about
a) 90°
b) 109°
c) 120°
d) 180°

The best predicted shape and bond angle of SbH 3 is
1. trigonal pyramidal; 107°.
2. trigonal pyramidal; 109.5°.
3. tetrahedral; 109.5°.
4. trigonal planar; 120°.

The bond angels in SF5+ are expected to be:
a. 90°
b. 120°
c. 90° and 120°
d. 90° and 180°
e. 90°, 120° and 180°

Which of the following molecules would have the smallest angles at the central atom?
A. CH4
B. NH3
C. H2O
D. CO2
E. PF5

Which of the following molecules or ions has the smallest H-N-H bond angle?
a) NH4+
b) NH3
c) NH2−
d) H2N-NH2
e) H2N-CH3

Which of the following has bond angles slightly less than 120 o?
NO3-
HO2-
NO2-
CS32-
I3+

The bond angle in NH3 is (smaller, larger) than the bond angle in CH4 because
1. smaller; nitrogen is smaller than carbon.
2. larger; the bond angles in trigonal planar molecules are larger than those in tetrahedral molecules.
3. smaller; the hybridization of nitrogen results in smaller bond angles than the hybridization of carbon.
4. smaller; the bond angles in trigonal planar molecules are smaller than those in tetrahedral molecules.
5. smaller; the unshared pair of electrons on nitrogen is more repulsive to the bonded electron pairs.
6. larger; the hybridization of nitrogen results in larger bond angles than the hybridization of carbon.
7. larger; nitrogen is larger than carbon.

What is the VSEPR geometry for CIO3-? _________________What is the molecular geometry = shape of CIO3-? ___________________Is CIO3- a polar or non-polar ion? ______________What is the approximate O-Cl-O bond angle in CIO3-? ______________

In cumulene, what are the C=C=C and H-C-H bond angles, respectively?Enter the C=C=C bond angle followed by the H-C-H bond angle separated by a comma.

What are the expected bond angles of ICl 4+? Choose all that apply:a) 90°b) 109.5°c) 120°d) 180°

What are the expected bond angles in ICl 4 + ? Check all that apply.
a) 90°
b) 109.5°
c) 120°
d) 180°

Predict the ideal bond angle(s) around each central atom in this molecule.

Predict the ideal bond angle(s) around each central atom in this molecule.

a. What is the molecular geometry of BrI 5? b. Ignoring lone-pair effects, what is the smallest bond angle in BrI 5? (Express your answer as an integer).

What is the value of the bond angles in CCl 4?

What is the value of the bond angle in ICl 2-?

PI3Cl2 is a nonpolar molecule. Based on this information, determine the I-P-I bond angle, the Cl-P-Cl bond angle, and the I-P-Cl bond angle.Enter the number of degrees of the I-P-I , Cl-P-Cl, and I-P-Cl bond angles, separated by commas (e.g., 30,45,90)

What is the value of the smallest bond angle in XeF 4?

What is the value of the bond angles in CH4, IF 4-, AlCl3, and I3?

How can I predict the bond angles for IF4−?

What are the expected bond angles in ICl4+?a. 90°b. 109.5°c. 120°d. 180 °

What is the value of the bond angles in SiCl 4?

What is the value of the bond angle in I 3-?

Consider the Lewis structure for glycine, the simplest amino acid: What are the approximate bond angles at the nitrogen?

Select the correct value for the indicated bond angle in each of the following compounds:

Based on the bond angles in CH4, NH3, and H2O. rank the magnitude of these repulsions. Rank from strongest to weakest repulsion. To rank items as equivalent, overlap them.

What are the expected bond angles of ICl 4+? Choose all that apply:a. 90 degreesb. 109.5 degreesc. 120 degreesd. 180 degrees

In cumulene (C4H4) , what are the C=C=C and H-C-H bond angles, respectively?

The molecular geometry of NO2- is, Use VSEPR to justify your answer.A) bent, bond angle - 109°B) trigonal planarC) linearD) bent, bond angle - 120°

Predict the ideal bond angle(s) around each central atom in this molecule.

What is the value of the bond angles in COH 2?

A molecule with a seesaw molecular geometry has a bond angle ofA) <120° for equatorial bonds and <90 degree for axial bondsB) 180°C) <90°D) 120° for equatorial bonds and 90° for axial bondsE) 120°

What would you expect to be the electron-group arrangement around atom A in the following case? Give the ideal bond angle. Electron-group arrangement:a. trigonal bipyramidalb. square planarc. trigonal planarIdeal bond angle: ____°

What is the value of the smallest bond angle in ClF 4-?

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