Chapter 1, Problem 71P

The element sulphur has atomic number 16. Sulphur forms a molecular compound with chloride with a molecular formula SCl2. The atomic number of chlorine is 17. a. Write down the electronic configuration of a sulphur atom and a chlorine atom. b. Draw a Lewis structure of an SCl2 molecule, by showing the electrons in the outer shells of the atoms. c. State how many bond pairs and lone pairs of electrons are arranged around the sulphur atoms in SCl2 molecule. d. Sketch the shape and state the molecular geometry of SCl2 molecule. e. Explain the hybridisation of the central atom in SCl2 molecule. f.Explain the intermolecular forces exists in SCl2 molecule.

1. Which statement about chemical bonds is true? a. It is an electrostatic attraction that holds two atoms together.b. It involves the combination of two nuclei of different atoms.c. It involves the temporary attraction between two or more substances.d. It deals with the physical separation of substances to form another set of substances.  2. Which Lewis electron-dot diagram represents a rubidium atom? a. Rb•b. :Rb•c. Rb:d. •Rb• 3. The bond between Br atoms in a Br2 molecule is _______ and is formed by the _________ of two valence electrons.  a. ionic ; sharingb. ionic ; transferc. covalent ; sharingd. covalent; transfer

Chemistry: Bonding 1. a. Identify and describe the type of bonding present in BaCl2. b. What is the electron configuration of the Ba after bonding? What is the electron configuration of the Cl after bonding?  c. Draw the Lewis structure of BaCl2

Draw a Lewis structure for BF3 that obeys the octet rule if possible and answer the following questions based on your drawing.      1. For the central boron atom:              - The number of lone pairs = ?              - The number of single bonds = ?              - The number of double bonds = ?      2. The central boron atom is              a. obeys the octet rule.              b. has an incomplete octet.              c. has an expanded octet.

a. Predict the formula of thecompound formed from aluminum and fluorine.b. Calculate the electronegativity difference between aluminum and fluorine.c. Is the AlF bond ionic, polar covalent, or nonpolar covalent?d. Write the name of the compound formed from aluminum and fluorine..e. Is this compound ionic, polar covalent, or nonpolar covalent?f. Is this compound water soluble?     ( give the  all answer with stepwise and type the answer.)

1. a. Identify and describe the type of bonding present in BaCl,. b. What is the electron configuration of the Ba after bonding? What is the electron configuration of the Cl after bonding? c. Draw the Lewis structure of BaCl,.

pls make sure it’s correct

No plagiarism Please 4. Based on the electron configuration what ion is most likely to form from these atoms? These substances are all three metals.  A. -1 B. +1 C. 0- Neutral D. none of these   5. Using the images from question 4, what type of bond is most likely to be formed by these ions? A. ionic B. covalent C. polar covalent D. nonpolar covalent

1. The electron pair in a H - Cl bond could be considered... a. closer to H because Hydrogen has a larger radius and thus exerts greater control over the shared electron pair b. closer to Cl because Chlorine has a higher electronegativity than Hydrogen c. closer to H because Hydrogen has a lower electronegativity than Chlorine d. an inadequate model since the bond is ionic 2. It is important to know the geometry of a molecule because the geometry _______.   a. will give the Lewis structure of the molecule b. affects the physical and chemical properties of the substance c. will determine whether the molecule is ionic or covalent d. Both B, and C