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Draw a valid Lewis structure for tetrafluoroethylene.
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Chemistry & Chemical Reactivity
- Acrylamide, H2C=CHCONH2, is a known neurotoxin and possible carcinogen. It was a shock to all consumers of potato chips and french fries a few years ago when it was found to occur in those products. (a) Sketch the molecular structure of acrylamide and identify all bond angles. (b) Indicate which carbon-carbon bond is the stronger of the two. (c) Is the molecule polar or nonpolar? (d) The amount of acrylamide found in potato chips is 1.7 mg/kg. If a serving of potato chips is 28 g, how many moles of acrylamide are you consuming?arrow_forwardNow, we will investigate diatomic molecules, those that are made up of two of the same type of atom. Select 2 fluorine atoms. How many valence electrons are in each fluorine atom? Is a fluorine atom a metal or a non-metal? Did the combination of these atoms create a covalent or ionic bond? How are the valence electrons organized to form a bond between these atoms? How is this different from the ionic bonds formed in the previous part of the activity?arrow_forwardwww TT In the first column type the number of atoms in the covalent compound. In the second column, type the total number of VALENCE electrons in the compound (all electrons: shared and unshared electrons). In the third column, determine the total number of possible chemical bonds in the compound. Compound H₂ Cl₂ 0₂ N₂ H₂O SF2 CH4 NH3 PF3 CC14 C₂H6 CHEMISTRY Covalent Compounds and Electrons Number of Atoms I Total Valence Electrons Total possible of chemical bondsarrow_forward
- Answer the questions in the table below about the shape of the sulfur tetrafluoride (SF4) molecule. How many electron groups are around the central sulfur atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central sulfur atom? (You may need to use the scrollbar to see all the choices.) 0 ✓ (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedralarrow_forwardDraw a horizontal bar that depicts the ability of atom to attract electrons in a chemical bond. Draw it on the space provided on the table. Take 1 cm to represent 2 values of electronegativity. Example: Hydrogen= 1.10: 0.55 cm, Fluorine: 4.00 2.00 cm 1 18 H 2 13 14 15 16 17 Li Be B O Mg Al S Ca Ga Se Sr In Te Na K Rb C Si Ge Sn N P As Sb F J Brarrow_forward0=C=0 Consider the model shown above. What type of bond is made by the elements and why? The bond will be ionic because carbon is a nonmetal and oxygen is a nonmetal. The formula will be CO2 because the charge on carbon is +4 and the charge on oxygen is -4. The bond will be covalent because carbon is a metal and oxygen is a nonmetal. The formula will be C20 because the charge on carbon is +4 and the charge on oxygen is -2. The bond will be covalent because both carbon and oxygen are nonmetals. The formula will be CO, because the electrons between the atoms are being shared equally. The bond will be ionic because both carbon and oxygen are nonmetals. The formula will be CO, because the electrons between the atoms are being shared unequally. 58°F Cleararrow_forward
- Part II: Binary Covalent Compounds Covalent compounds are produces by nonmetals bonding with one another. You can use the valence electrons for each element to determine the simplest formula that exists between two elements. For example, H has 1 valence electron and needs one more to obey the Octet Rule, so it will only make 1 bond when found in a compound. Oxygen has 6 valence electrons and needs two more to obey the Octet Rule, so it typically makes 2 bonds when found in a compound. Since hydrogen needs just one electron while oxygen needs two, the correct formula for the simplest compound would be H20. However, there are often other combinations possible in addition to the simplest formula. For example, hydrogen and oxygen can also form, H2O2, which is known as hydrogen peroxide. To work with all the possible combinations, some rules have been developed for naming binary covalent compounds. The rules are stated below: 1. The least metallic element will always end in the suffix…arrow_forwardDecide whether these proposed Lewis structures are reasonable. proposed Lewis structure Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: Н — Н — О No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: 0=0= O No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: Н — СС — Н No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "O,0". :0: :0: :0 :arrow_forwardQ 5. Define electronegativity. Use electronegativity (EN) values to determine whether the bonds between the following atoms are non polar covalent, polar covalent or ionic (calculations must be shown) a) C (EN = 2.55) and H (EN = 2.20) b) K (EN = 0.82) and F (EN = 3.98) c) H (EN = 2.20) and Br (EN = 2.96) d) Mg (EN = 1.31) and Cl (EN = 3.16)arrow_forward
- Draw an acceptable Lewis structure for each compound, assuming the atoms are connected as arranged. Formaldehyde (H2CO) is a preservative, and glycolic acid (HOCH2CO2H) is used to make dissolving sutures.arrow_forwardCompounds such as Freon® 112 (referred to as chlorofluorocarbons, or CFCs) were used as refrigerants for many years, but they were phased out because of their harmful effects on Earth's atmosphere. Write the molecular and empirical formulas for Freon 112. The Lewis dot structure of Freon 112. There are two central carbon atoms bonded together through a single bond. Each carbon atom is bonded to two chlorine atoms and one fluorine atom through single bonds. Each chlorine atom has 3 lone pairs. Each fluorine atom has 3 lone pairs.arrow_forwardAll About Covalent Bonds When atoms react to form more stable compounds, it is the unpaired valence electrons that are used to make a bond. In a covalent bond, the unpaired valence electrons are shared. When a stable molecule is made, each atom will have 8 valence electrons (except for period 1 elements, which will have 2 valence electrons).arrow_forward
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