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What is the geometry of molecule having one lone and three bond pairs?
Wiki User
∙ 11y ago
Trigonal pyramidal
Wiki User
∙ 11y ago
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How do you determine the molecular geometry of a molecule?
The molecular geometry of a molecule can be determined using the VSEPR theory. VSEPR (Valence Shell Electron Pair Repulsion) Theory: The basic premise of this simple theory is that electron pairs (bonding and nonbonding) repel one another; so the electron pairs will adopt a geometry about an atom that minimizes these repulsions. Use the method below to determine the molecular geometry about an atom. Write the Lewis dot structure for the molecule. Count the number of things (atoms, groups of atoms, and lone pairs of electrons) that are directly attached to the central atom (the atom of interest) to determine the overall (electronic) geometry of the molecule. Now ignore the lone pairs of electrons to get the molecular geometry of the molecule. The molecular geometry describes the arrangement of the atoms only and not the lone pairs of electrons. If there are no lone pairs in the molecule, then the overall geometry and the molecular geometry are the same. If the overall geometry is tetrahedral, then there are three possibilities for the molecular geometry; if it is trigonal planar, there are two possibilities; and if it is linear, the molecular geometry must also be linear. The diagram below illustrates the relationship between overall (electronic) and molecular geometries. To view the geometry in greater detail, simply click on that geometry in the graphic below. Although there are many, many different geometries that molecules adopt, we are only concerned with the five shown below.
Why is the molecular geometry of PH3 trigonal pyramidal?
In having three hydrogens attached to a phosphorous atom the arrangement is forced as the lone pairs must be kept as far from each other as possible, thus the geometry here.
What is the electron-pair geometry for SeOF2?
SeOF2 is known as Selenyl Difluoride. The Se atom has one pair of electrons, each F atom has three pairs, and the O has two pairs of electrons.
Which one of the following describes the molecular geometry of a molecule with four electron groups with only bonded pairs?
tetrahedral, if it had three electron groups it would be trigonal planar
What is the molecular geometry of PF3?
In a molecule of phosphorus fluoride, the phosphorus atom is in the center, and it is surrounded by the three fluoride atoms which are arranged at three of the four points of a tetrahedron. (The fourth point of the tetrahedron contains an electron pair from the phosphorus atom.)
How do you determine the molecular geometry of a molecule?
The molecular geometry of a molecule can be determined using the VSEPR theory. VSEPR (Valence Shell Electron Pair Repulsion) Theory: The basic premise of this simple theory is that electron pairs (bonding and nonbonding) repel one another; so the electron pairs will adopt a geometry about an atom that minimizes these repulsions. Use the method below to determine the molecular geometry about an atom. Write the Lewis dot structure for the molecule. Count the number of things (atoms, groups of atoms, and lone pairs of electrons) that are directly attached to the central atom (the atom of interest) to determine the overall (electronic) geometry of the molecule. Now ignore the lone pairs of electrons to get the molecular geometry of the molecule. The molecular geometry describes the arrangement of the atoms only and not the lone pairs of electrons. If there are no lone pairs in the molecule, then the overall geometry and the molecular geometry are the same. If the overall geometry is tetrahedral, then there are three possibilities for the molecular geometry; if it is trigonal planar, there are two possibilities; and if it is linear, the molecular geometry must also be linear. The diagram below illustrates the relationship between overall (electronic) and molecular geometries. To view the geometry in greater detail, simply click on that geometry in the graphic below. Although there are many, many different geometries that molecules adopt, we are only concerned with the five shown below.
What is the electronic geometry of bi3?
What is the electronic geometry of Bi_3? Enter the ... Thus, the total number of electrons in the molecule will be 24. There are no lone pairs in boron. Three electron domains are thus present in this molecule. Therefore, the electronic geometry of B I 3 is trigonal planar.
Why is the molecular geometry of PH3 trigonal pyramidal?
In having three hydrogens attached to a phosphorous atom the arrangement is forced as the lone pairs must be kept as far from each other as possible, thus the geometry here.
How many unshardd pairs of electrons are in a molecule of hydrogen iodide?
There would be three unshared pairs of electrons in a molecule of hydrogen iodide.
What is the Lewis dot diagram for silicon tetrachloride?
VSEPR stands for Valence Shell Electron Pair Repulsion, and this name is extremely descriptive. It means, in essence, that pairs of electrons (whether bonding pairs or lone, non-bonding pairs) repel one another due to their negative electric charges. As a result, molecules tend to assume a geometry that maximizes the angular separation between electron pairs. The simplest case is methane, CH4. There are four bonding pairs of electrons around the central carbon atom. Thus, they will tend to repel one another such that the four H's achieve maximum angular separation. It turns out that this geometry is that of a tetrahedron, with an angular separation of about 109.5°. A very similar but slightly more complicated molecule is NH3, ammonia. There are three bonding pairs and one lone, non-bonding pair of electrons around the central nitrogen atom. As we saw in methane, this causes ammonia to assume a tetrahedral geometry for maximum angular separation of electron pairs. However, it turns out that lone, non-bonding pairs exert a greater repulsion than do bonding pairs. This causes the three bonding pairs to push a little bit closer together, for an angular separation of about 107.8° rather than 109.5°. A good rule of thumb is that each lone pair pushes the bonding pairs together by about 2°. Technically speaking, ammonia is not a tetrahedral molecule, because we do not consider lone pairs when describing a molecule's geometry. Instead, we consider only the N-H bonds, and call ammonia a pyramidal molecule. Next, we consider H2O, water. The central oxygen atom has two bonding pairs of electrons, and two lone pairs of electrons. The tetrahedral geometry is upset by these two lone pairs, pushing the O-H bonds together to an angular separation of about 104.5° (two lone pairs, so about 4° closer). The geometry of the molecule, not counting lone pairs, is thus said to be "bent." BH3, borane, is an unusual molecule. Because boron has only three valence electrons, it tends to form three bonds. Borane thus has three bonding pairs of electrons, and no lone pairs, causing it to assume a trigonal planar geometry. The angular separation is thus 120°. CO2, carbon dioxide, is a very simple case. The central carbon atom forms two double bonds, with two bonding pairs of electrons on each side. Its geometry is therefore linear. There are some other geometries, but they are very special cases, and only occur in unusual compounds. XeF6, xenon hexafluoride, for example, assumes an octahedral geometry; PCl5, phosphorus pentachloride, assumes a trigonal bipyramidal geometry; SF4, sulfur tetrafluoride, assumes a see-saw geometry; ClF3, chlorine trifluoride assumes a T-shaped geometry; XeF4, xenon tetrafluoride, assumes a square planar geometry; ClF5, chlorine pentafluoride assumes a square pyramidal geometry. Look these compounds up in Wikipedia for images and explanations. Now, to answer your questions. Silicon and chlorine are both non-metals, meaning that silicon tetrachloride is a molecular compound (i.e. one that has covalent bonds). To draw the Lewis structure of it, you'd simply draw Si in the middle, and four Cl's projecting outwards. If you're drawing the full 3D geometry, you'd draw something like the first link below. If you're drawing the flat, planar Lewis structure, you'd draw something like the second link below. Next, let's consider what VSEPR says about SCl2. We'll assume that sulfur is the central atom. It is a group VIA element, like oxygen, so it has six valence electrons. By forming two single bonds (one to each chlorine), it fills its octet. We would thus predict two pairs of bonding electrons, and two lone pairs. The four pairs would orient themselves in roughly tetrahedral fashion (although the lone pairs would push the bonding pairs about 4° closer together, to about 104.5°). The molecule's geometry, excluding lone pairs, would thus be bent like that of water. This molecule is clearly polar, because it has no internal symmetry. C2Cl2, on the other hand, is a more complicated example. This molecule is called dichloroethyne, having a triple bond between the two carbon atoms, with a single C-Cl bond on each side. This molecule thus has a linear geometry (180° bond angles), with no need to resort to VSEPR. Since linear molecules are symmetrical, it is non-polar even though it contains highly polar bonds.
What is the molecular geometry of clo3?
Trigonal planar because it has three bonding pairs and one lone pair
What is anticondon?
An anticodon is the three-base sequence on a tRNA molecule that pairs with a specific mRNA codon.
What are the three of the many possible shapes of molecules?
Without given a specific molecule there is not any way to determine the shape. Beryllium chloride consists of beryllium in the middle and a chlorine on each side, and is in the shape of a straight line.
What is the origin of insects?
An insect is any animal of the class Insecta. They are normally small arthropods having the body divided into three parts, and having three pairs of legs and usually two pairs of wings.
What is the electron-pair geometry for SeOF2?
SeOF2 is known as Selenyl Difluoride. The Se atom has one pair of electrons, each F atom has three pairs, and the O has two pairs of electrons.
Why is aluminium trichloride molecule non polar but the bonds in it are polar?
Because of the geometry/symmetry of the molecule. The three Cl atoms are arranged in such a way that the charge distribution is equal, thus making the molecule non polar.
What is the shape of a molecule which has three shared pairs of electrons and no unshared pairs?
The molecule is likely to have a trigonal planar shape, where the three shared electron pairs are arranged symmetrically around the central atom, creating a flat triangle. This results in an angle of 120 degrees between each electron pair.
