Identify each of the following molecules as polar or nonpolar:
Drag the appropriate items to their respective bins.
РВгз
SeF2
SiF 4
CHCl3
Polar: CHCl3
Nonpolar: РВгз, SeF2, SiF4
To determine whether a molecule is polar or nonpolar, we need to look at the molecular geometry and the presence of any molecular dipoles.
1) РВгз:
Unfortunately, the molecule "РВгз" is not recognized as a valid chemical formula. Please provide the correct formula.
2) SeF2:
The central atom in SeF2 is selenium (Se), with two surrounding fluorine atoms (F). Since there are two lone pairs on the selenium atom and the molecule has a bent shape, the bond polarities do not cancel each other out. Therefore, SeF2 is a polar molecule.
3) SiF4:
The central atom in SiF4 is silicon (Si), with four surrounding fluorine atoms (F). Since the molecule has a tetrahedral shape, with the four fluorine atoms symmetrically arranged around the central silicon atom, the bond polarities cancel each other out. Therefore, SiF4 is a nonpolar molecule.
4) CHCl3:
The central atom in CHCl3 is carbon (C), with three surrounding hydrogen atoms (H) and one chlorine atom (Cl). Since the molecule has a tetrahedral shape, with the three chlorine atoms arranged asymmetrically around the central carbon atom, the bond polarities do not cancel each other out. Therefore, CHCl3 is a polar molecule.
To identify whether a molecule is polar or nonpolar, we need to consider the molecular geometry and the polarity of individual bonds within the molecule.
1. РВгз: To determine the polarity of this molecule, we need to know its structure. Unfortunately, "РВгз" does not provide enough information about the arrangement of atoms. Can you please provide more details or clarify the molecule's name?
2. SeF2: Selenium difluoride (SeF2) consists of one selenium atom bonded to two fluorine atoms. In this case, selenium (Se) is the central atom with two regions of electron density (lone pairs and bond pairs) and two fluorine atoms as the terminal atoms. The molecular geometry of SeF2 is bent or V-shaped due to the presence of two lone pairs on the selenium atom. Since the lone pairs do not cancel out, the molecule is polar.
3. SiF4: Silicon tetrafluoride (SiF4) has a silicon atom in the center bonded to four fluorine atoms. The molecular geometry of SiF4 is tetrahedral, with no lone pairs on the central silicon atom. Since the fluorine atoms are arranged symmetrically around the central silicon, the bond dipoles cancel each other out, resulting in a nonpolar molecule.
4. CHCl3: Chloroform (CHCl3) consists of one carbon atom bonded to three hydrogen atoms and one chlorine atom. The molecular geometry of CHCl3 is tetrahedral, where three chlorine atoms surround the central carbon atom, along with one hydrogen atom. Since the chlorine atoms are more electronegative than the carbon atom, the C-Cl bonds have a slight dipole moment. Additionally, due to the tetrahedral shape and the unequal distribution of the dipoles, the molecule is polar.
In summary:
- РВгз: More information or clarification is needed to determine its polarity.
- SeF2: Polar
- SiF4: Nonpolar
- CHCl3: Polar