Concept explainers
(a)
Interpretation:
Interpret and complete the given statement.
There are − electron group around the central Se atom.
Concept Introduction:
Lewis dot structure is the representation of the atom bonded to each other to form a molecule or compound.
The bond formation between the atoms takes place due to the sharing of valence electrons between them while the remaining outer electron denoted as lone pair of electrons.
(b)
Interpretation:
Interpret and complete the given statement.
The electron group geometry is −
Concept Introduction:
Lewis dot structure is the representation of the atom bonded to each other to form a molecule or compound.
The bond formation between the atoms takes place due to the sharing of valence electrons between them while the remaining outer electron denoted as lone pair of electrons.
(c)
Interpretation:
Interpret and complete the given statement.
The number of atoms attached to the central se atom is −
Concept Introduction:
Lewis dot structure is the representation of the atom bonded to each other to form a molecule or compound.
The bond formation between the atoms takes place due to the sharing of valence electrons between them while the remaining outer electron denoted as lone pair of electrons.
(d)
Interpretation:
Interpret and complete the given statement.
The shape of the molecule is-
Concept Introduction:
Lewis dot structure is the representation of the atom bonded to eachother to form a molecule or compound.
The bond formation between the atoms takes place due to the sharing of valence electrons between them while the remaining outer electron denoted as lone pair of electrons.
Want to see the full answer?
Check out a sample textbook solutionChapter 10 Solutions
EBK BASIC CHEMISTRY
- For each molecule below, a. Draw the lewis structure, using wedges and dashes to indicate the VSEPR shape as necessary. b. Draw the bond dipole for all polar bonds. c. Determine if the overall molecule is polar or nonpolar. first molecule: H₂ second molecule: CO₂ third molecule: H₂Oarrow_forwardQuestion 48 48. Which of the following statements are true? 1. 11. III. IV. The electrons in each molecule tend to orient themselves around the most electronegative element. Each molecular drawing follows the localized electron model. Both HF and CO₂ are linear molecules and therefore polar. The bond angles of NH3 are slightly less than 109.5° because the lone pair compresses the angles between the bonding pairs. a. I, III, IV b. I, II, IV c. I, II, III d. II, IV e. All of the above statements are correct. C B esc E Q @ 2 W # 3 E $ 4 * R % 5 T < 6 Y & 7 8 Uarrow_forwardPart II Practicing Coordinate Covalent Bonding for Molecular compounds. Example: Given the molecular compound SO, draw the molecular compound using the coordinate covalent bonding model. A. Calculate the total number of electrons. S = 1x 6 = 6 electrons O = 4 x 6 = 24 electrons Charge -2 = 2 electrons Total = 32 electrons B. Determine Center Atom (look for the single element) in this case S. C. Now make a single bond to all other elements to the central atom. You have used 8 electrons of the 32. 0- D. Place electrons around the atoms that are bonded to the central atom so that each will have 8 electrons around them (in this case each oxygen needs 6 more electrons or 3 pairs of electrons). : E. Make sure that the central atom has a full octet (8 electrons). In this case it does, so you are done. If not, one of the lone pairs of electrons from an outer atom will share a second pair of electrons with the center atom. Finally be sure that you have used all your electrons and NO MORE!arrow_forward
- Which element would form a Covalent (Molecular) bond with Carbon (C) ? a. 5 Tellurium (Te) b. 9 Nitrogen (N) c. Neither Name of this molecule: ________________________________________ 3. Which element would form a Covalent (Molecular) bond with Chlorine (Cl) ? a. 3 Calcium (Ca) b. 7 Sulfur (S) c. Neither Name of this molecule: ________________________________________ 4. Which element would form a Covalent (Molecular) bond with Xenon (Xe)? a. 8 Francium (Fr) b. 1 Hydrogen (H) c. Neither Name of this molecule: ________________________________________ 5. Which element would form a Covalent (Molecular) bond with Hydrogen (H)? a. 7 Fluorine (F) b. 8 Argon (Ar) c. Neither Name of this molecule: ________________________________________arrow_forward2. For each of the following compounds: a. Draw a Lewis structural diagram b. Using electronegativity, predict whether bonds will be polar or nonpolar c. Using bond polarity and shape, predict whether the molecule will be polar or nonpolar Identify the greatest Intermolecular force present d. Molecule CS₂ NH, Structural Diagram (include bond polarity and partial or full charges) Bond Type (ionic/polar covalent/ nonpolar covalent) Molecule Type (ionic/polar /nonpolar) Intermolecular Forcearrow_forwardAnswer the following questions about the molecule Cl 2O. a. How many valence electrons does Cl 2O contain? b. Draw a valid Lewis structure. c. Label all polar bonds. d. What is the shape around the O atom? e. Is Cl 2O a polar molecule? Explain.arrow_forward
- 3. The electron dot diagram for a neutral atom of chlorine (atomic number 17) is shown below. Which of the following symbols represents a chlorine ion with a stable arrangement of eight valence electrons? :CI : O A. 35CI1- O B. 35C12- O . 35C1+ O D. 35CIarrow_forwardA. Draw the Lewis Dot Structure of the molecule or ion OF2 B. Find the shape of the molecule or ion OF2 C. Draw the Lewis Dot Structure of the molecule or ion CH2F2 D. Find the shape of the molecule or ion CH2F2 E. Draw the Lewis Dot Structure of the molecule or ion PO3^-3 F. Find the shape of the molecule or ion PO3^-3arrow_forwardchlorine 1. Electronegativity values increase from left to right across a period in the periodic table because smaller there is an increase in the charge of the nuclei in this direction. iodine 2. These values also increase from the bottom to the top of a group because the size of the atom carbon decreases, resulting in a distance between the nucleus and the valence electron shell, which increases the attraction between the protons and electrons. positive negative 3. When considering both carbon and oxygen, is more electronegative because it appears further to the right in the same period of the periodic table. oxygen larger 4. When considering chlorine and iodine, is more electronegative because it appears higher in the same group of the periodic table. M acerarrow_forward
- For the following molecules, NF3 a. Give the total number of valence electrons in the moleculeb. Draw the lewis structurec. Name the molecule using the proper naming system for covalent molecules.d. Identify the electron geometry and the molecular geometry (shape)e. Give the electronic configurations for carbon, chlorine and fluorine. Identify anysimilarities.f. Find another molecule that has the same molecular geometry (the shape) as NF3arrow_forwardCompare the two molecules (I. and II.) below on the various aspects of molecular shape and related properties given. 1. SeCl4 11. SC12 (in both compounds, the letter after C is an L, not i) > DOD has a larger bond angle has double or triple bonds electron group arrangement is the same as the molecular shape central atom contains 1 or more lone pairs flat, two-dimensional shape polar molecule 1. only I. 2. only II. 3. both molecules 4. neither moleculesarrow_forwardCAELLE PIERRE - LAB 16: COVALENT AND IONIC COMPOUNDS Summary lonic Compounds versus Covalent Compounds How are covalent compounds different How are ionic compounds different from covalent compounds? How are ionic and covalent compounds similar? from ionic compounds? 1. 1. 1. 2. 2. 2. 3. 3. 3. SAMSUNG 女 & % @ 23 3 y W e k d. a Sarrow_forward
- Chemical Principles in the LaboratoryChemistryISBN:9781305264434Author:Emil Slowinski, Wayne C. Wolsey, Robert RossiPublisher:Brooks Cole