1. For the following group of elements: Nitrogen (N), Hydrogen (H), Sulfur (S). Nitrogen has an atomic number of 7, and electronegativity of 3.04. Hydrogen has an atomic number of 1, and an electronegativity of 2.20. Sulfur has an atomic number of 16 and an electronegativity of 2.58. a. Draw the electron configuration diagrams for each element shown. b. Draw a molecule that could be made using these elements. Do not worry about whether the molecule is actually stable in nature, just try to fill the electron shells. You have to use all of the elements in your molecule, but you can use any element more than once. c. Label each bond as non-polar, polar, or ionic. Show the partial or full charges.

1. For the following group of elements: Nitrogen (N), Hydrogen (H), Sulfur (S). Nitrogen has an atomic number of 7, and electronegativity of 3.04. Hydrogen has an atomic number of 1, and an electronegativity of 2.20. Sulfur has an atomic number of 16 and an electronegativity of 2.58. a. Draw the electron configuration diagrams for each element shown. b. Draw a molecule that could be made using these elements. Do not worry about whether the molecule is actually stable in nature, just try to fill the electron shells. You have to use all of the elements in your molecule, but you can use any element more than once. c. Label each bond as non-polar, polar, or ionic. Show the partial or full charges.

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 3STP

See similar textbooks

Similar questions

Determining Molecular Polarity Determine whether each molecule is polar: a.HBrb.IClc.I2d.CO
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
Which of the following best describes electronegativity trends in the periodic table?I. Electronegativity inreases from right to left across a period.II. Electronegativity inreases from left to right across a period.III. Electronegativity inreases from bottom to top within a group.IV. Electronegativity inreases from top to bottom within a group. Select one: a. I and III b. I and IV c. II and III d. II and IV e. None of these.
Which of the following best describes electronegativity trends in the periodic table? I. Electronegativity inreases from right to left across a period. II. Electronegativity inreases from left to right across a period. III. Electronegativity inreases from bottom to top within a group. IV. Electronegativity inreases from top to bottom within a group. Select one: O a. I and IlI b. I and IV c. Il and III d. Il and IV e. None of these.
Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for NH,* and answer the following questions based on your drawing. 1. For the central nitrogen atom: The number of lone pairs The number of single bonds = The number of double bonds= 2. The central nitrogen atom A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet.
ionic character of the bond is less than 51% percent so the bond is covalent. (Think and check the periodic table) Multiple Choice. 20. In the molecule models of HF, HCI, and HBr on page 10, the respective numbers (1.0cm, 1.2 cm, and 1.5 cm) represent the a. protons in the atom c. repulsive force between the atoms b. molecular distance between nuclei d. actual distance between atoms 21. The halogen element that has the most attraction for the hydrogen electron is a. fluorine b. chlorine c. bromine
9. Use table of electronegativities to determine the bond formed between Sulfur & Fluorine a. ionic b. polar covalent c. nonpolar covalent d. none of these 10. Use table of electronegativities to determine the bond formed b/w Potassium & Chloride a. ionic b. polar covalent c. nonpolar covalent d. none of these 11. Use table of electronegativities to determine the bond formed b/w Nitrogen & Silicon a. ionic b. polar covalent c. nonpolar covalent d. none of these 12. Use table of electronegativities to determine the bond formed b/w Hydrogen & Sulfur a. ionic b. polar covalent c. nonpolar covalent d. none of these 13. Use table of electronegativities to determine the bond formed b/w Oxygen & Phosphorus a. ionic b. polar covalent c. nonpolar covalent d. none of these 14. What does it mean if a molecule has a polar covalent bond? a. one atom of the molecule is more electronegative that the other b. each atom of the molecule has the same electronegativity the molecule basa double bond &
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.)
Beaulac Highline CHEM& 121 6) Double and triple bonds form because a. the atoms involved have high electronegativities. b. single covalent bonds do not give all of the atoms in the molecule 8 valence electrons. C. one of the atoms in the molecule has more than 8 valence electrons. d. the ions involved have charges larger than one. 0) Group IIA metals form ions with a charge. 8) Group VA nonmetals form ions with a charge. ) Group VIIA nonmetals form ions with a charge. ) List the metals not in group IA or IIA that only form one ion. ) Fill in the blanks in the following table: Polyatomic Ion Chemical Formula Polyatomic Ion Chemical Formula sulfate chlorate NO2 ammonium perbromate PO,3- CIO- nitrate bicarbonate cyanide iodite OH carbonate
For question 2, bond types include... 1. covalent (slightly polar) 2. covalent (pure) 3. ionic 4. polar covalent
A covalent bond is likely to be polar when ________. a. one of the atoms sharing electrons is more electronegative than the other atom b. the two atoms sharing electrons are equally electronegative c. carbon is one of the two atoms sharing electrons d. the two atoms sharing electrons are of the same elements
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.