a) ClF4- has a square planar geometry due to its five electron domains, with four bonding pairs and one lone pair. b) ClF4+ has a linear geometry with no lone pairs, resulting in a linear molecular shape. c) NO2- has a T-shaped geometry with three electron domains - one lone pair and two bonding pairs. d) BrF3 has a bent molecular geometry due to the presence of two lone pairs and two bonding pairs around the central atom. e) CO2 has a linear molecular geometry as it has two electron domains and no lone pairs around the central carbon atom.
The Lewis structure for the ClF2O2⁺ ion involves a chlorine (Cl) atom at the center, bonded to two fluorine (F) atoms and two oxygen (O) atoms. Chlorine has seven valence electrons, and in this structure, it forms single bonds with the two fluorine atoms and each oxygen atom, using four of its valence electrons. The positive charge on the ion indicates that one electron is missing, which can be accounted for by the chlorine atom having fewer electrons available for bonding. The structure should also reflect that oxygen typically has two lone pairs, while fluorine has three lone pairs each.
OH alone would be linear shape AX1E3 bond angle 180o
Trigonal Pyramidal - 107.5 degrees It has 3 bonds and one lone pair. With all 4 elements (the 3 covalent bonds plus the lone pair) you would think it was Tetrahedral, with 109.5 degrees between them, but because the lone pair is there, it pushes the other bonding electrons closer together and thus you have a smaller angle of 107.5 degrees and the different shape.
1 Source: My online chemistry book.
The SF3+ molecule has a T-shaped molecular geometry, with three bonding pairs and two lone pairs around the sulfur atom.
a) ClF4- has a square planar geometry due to its five electron domains, with four bonding pairs and one lone pair. b) ClF4+ has a linear geometry with no lone pairs, resulting in a linear molecular shape. c) NO2- has a T-shaped geometry with three electron domains - one lone pair and two bonding pairs. d) BrF3 has a bent molecular geometry due to the presence of two lone pairs and two bonding pairs around the central atom. e) CO2 has a linear molecular geometry as it has two electron domains and no lone pairs around the central carbon atom.
4 bond pairs (F-N=N-F) plus 3 lone pairs on each fluorine and 1 on each nitrogen:together 8 lone pairs plus 4 bond pairs in both cis- and trans-Dinitrogen difluoride
EDTA has 6 lone pairs of electrons four from oxygen atoms and two from lone pairs on nitrogen. IN complex ions all boncds are dative covalent so both electrons come from the ligand ion this case edta. so the answer is 6 electron pairs (12 electrons) are added
The molecular shape for ( \text{PH}_4^+ ) (phosphonium ion) is tetrahedral. This is because phosphorus has four bonding pairs around it, which results in a geometry with bond angles of approximately 109.5 degrees.
There are infinitely many in each of the two curves/lines.
The Lewis structure for the ClF2O2⁺ ion involves a chlorine (Cl) atom at the center, bonded to two fluorine (F) atoms and two oxygen (O) atoms. Chlorine has seven valence electrons, and in this structure, it forms single bonds with the two fluorine atoms and each oxygen atom, using four of its valence electrons. The positive charge on the ion indicates that one electron is missing, which can be accounted for by the chlorine atom having fewer electrons available for bonding. The structure should also reflect that oxygen typically has two lone pairs, while fluorine has three lone pairs each.
OH alone would be linear shape AX1E3 bond angle 180o
A lone neutron spontaneously decays into a proton plus an electron plus an antineutrino (to carry off extra energy).
They are the coordinates of the infinitely many points on the line defined by the equation.
Group the numbers in pairs. You have ten pairs, each of which is equal to -1 and the ten are to be added together. Total = -10
2x plus 3y