1. Can you help me what does mean for the Valence Shell Electron Pair Repulsion (VSEPR) Theory and examples too? 2. Can you help me with the explanation of the diatomic molecule, small molecule, large molecule and examples too?
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1. Can you help me what does mean for the Valence Shell Electron Pair Repulsion (VSEPR) Theory and examples too?
2. Can you help me with the explanation of the diatomic molecule, small molecule, large molecule and examples too?
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Solved in 3 steps
- How many valence electrons does a neutral a. K atom have? b. C atom? N atom? O atom?Plot the relative bond lengths for diatomic molecules as a function of size for the first row of elements on the next page.Could someone help me?? The answer to this question must look similar to the example attached. Back ground info: Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron…
- Can you help me with the SO2 step-by-step for number (Step 6)? I need help with the central atom surrounded by an identical electron group. I need help with the molecule polar.A model for BrF3 is shown in the Jmol window. BrF3 has T-shaped geometry. ball & stick ✔ - + labels Use the References to access important values if needed for this question. Rotate the molecule until you have a feeling for its three-dimensional shape. How many F atoms are bonded to the central Br atom? Are all of the positions about the central atom equivalent, or are there two kinds of positions? A T-shaped molecule can be derived from a trigonal bipyramidal molecule by removing two of the outer atoms. Would the atoms removed be both axial, both equatorial, or one of each? What approximate angle at the Br atom does the unique F atom make with either of the other two F atoms? ✓ degrees. For practice, type in the name of the geometry of the molecule:What is the name of this type of molecular structure?? I need help answering this question because I don’t know what format it’s called
- 4. Lewis dot structures are good tools for showing the arrangement of valence electrons in a molecule. They don't however convey correct information about the shape of a molecule. A student described the shapes of the molecules shown below. Both are incorrect. Write an explanation for this student explaining what he did wrong and giving the correct shape of each molecule based on VSEPR theory. Lewis Structure Student identified molecule geometry as... Н—О—H Linear WATER H H:C:H Square planar H МЕТHANEIn the actual molecule of which this is a Lewis structure, which of the labeled distances can change? unmarked marked You can click the "unmarked" tab to see the molecule without any of the distances marked. List all the distances that can change. For example, suppose all the distances were measured at a certain time, and again 0.1s later. If distance A might be 50% bigger or smaller the second time, but all the other distances are certain to be the same, you should write "A". If A and B might be different the second time, but no other distances, you would write "A, B. And so on. Note for advanced students: you can assume the molecule is dissolved in an appropriate solvent at room temperature. 0Only can be one or the other not both
- How do you know when to draw a solid wedge vs a dashed wedge when drawing 3D bond-line structures? I know that solid-wedge means the atom is pointing towards you and dashed wedge means it's in the back, but how do you know which atoms are in the front as opposed to the back? How can you tell what the configuration will look like in space just by looking at the lewis structure or name?A model for SiH4 is shown in the chem3D window. SiH4 has tetrahedral geometry. ball & stick |+ labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? If you take any three of the outer atoms, what shape do they define? | Consider the bond angles at the central atom. Do they all have the approximately the same numerical value? What is the approximate numerical value of this angle? | degrees. Are all four positions about the central atom equivalent, or is one of them different from the other three. For practice, type in the name of the geometry of the molecule: Previous NextIn the actual molecule of which this is a Lewis structure, which of the labeled distances can change? marked unmarked H A B You can click the "unmarked" tab to see the molecule without any of the distances marked. H H. List all the distances that can change. For example, suppose all the distances were measured at a certain time, and again 0.1s later. If distance A might be 50% bigger or smaller the second time, but all the other distances are certain to be the same, you should write "A". If A and B might be different the second time, but no other distances, you would write "A, B". And so on. Note for advanced students: you can assume the molecule is dissolved in an appropriate solvent at room temperature. OO,... ?