name of [(1,1-dimethyl-2-propynyl)oxy]trimethylsilane

[(1, 1-dimethyl-2-propynyl)oxy]trimethylsilane

molar mass | 156.3 g/mol formula | C_8H_16OSi empirical formula | C_8O_Si_H_16 SMILES identifier | C#CC(C)(C)O[Si](C)(C)C InChI identifier | InChI=1/C8H16OSi/c1-7-8(2, 3)9-10(4, 5)6/h1H, 2-6H3 InChI key | JNRUXZIXAXHXTN-UHFFFAOYSA-N

Draw the Lewis structure of [(1, 1-dimethyl-2-propynyl)oxy]trimethylsilane. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4), hydrogen (n_H, val = 1), oxygen (n_O, val = 6), and silicon (n_Si, val = 4) atoms: 8 n_C, val + 16 n_H, val + n_O, val + n_Si, val = 58 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), oxygen (n_O, full = 8), and silicon (n_Si, full = 8): 8 n_C, full + 16 n_H, full + n_O, full + n_Si, full = 112 Subtracting these two numbers shows that 112 - 58 = 54 bonding electrons are needed. Each bond has two electrons, so in addition to the 25 bonds already present in the diagram add 2 bonds. To minimize formal charge carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |

longest chain length | 6 atoms longest straight chain length | 6 atoms longest aliphatic chain length | 4 atoms aromatic atom count | 0 atoms H-bond acceptor count | 1 atom H-bond donor count | 0 atoms

Find the elemental composition for [(1, 1-dimethyl-2-propynyl)oxy]trimethylsilane in terms of the atom and mass percents: atom percent = N_i/N_atoms × 100% mass percent = (N_im_i)/m × 100% Plan: • Write the chemical formula and gather atomic masses from the periodic table. • Determine values for N_i, m_i, N_atoms and m using these items. • Finally, compute the percents and check the results. Write the chemical formula: C_8H_16OSi Use the chemical formula to count the number of atoms, N_i, for each element and find the total number of atoms, N_atoms, per molecule: | number of atoms C (carbon) | 8 O (oxygen) | 1 Si (silicon) | 1 H (hydrogen) | 16 N_atoms = 8 + 1 + 1 + 16 = 26 Divide each N_i by N_atoms to calculate atom fractions. Then use the property that atom fractions must sum to one to check the work: | number of atoms | atom fraction C (carbon) | 8 | 8/26 O (oxygen) | 1 | 1/26 Si (silicon) | 1 | 1/26 H (hydrogen) | 16 | 16/26 Check: 8/26 + 1/26 + 1/26 + 16/26 = 1 Compute atom percents using the atom fractions: | number of atoms | atom percent C (carbon) | 8 | 8/26 × 100% = 30.8% O (oxygen) | 1 | 1/26 × 100% = 3.85% Si (silicon) | 1 | 1/26 × 100% = 3.85% H (hydrogen) | 16 | 16/26 × 100% = 61.5% Look up the atomic mass, m_i, in unified atomic mass units, u, for each element in the periodic table: | number of atoms | atom percent | atomic mass/u C (carbon) | 8 | 30.8% | 12.011 O (oxygen) | 1 | 3.85% | 15.999 Si (silicon) | 1 | 3.85% | 28.085 H (hydrogen) | 16 | 61.5% | 1.008 Multiply N_i by m_i to compute the mass for each element. Then sum those values to compute the molecular mass, m: | number of atoms | atom percent | atomic mass/u | mass/u C (carbon) | 8 | 30.8% | 12.011 | 8 × 12.011 = 96.088 O (oxygen) | 1 | 3.85% | 15.999 | 1 × 15.999 = 15.999 Si (silicon) | 1 | 3.85% | 28.085 | 1 × 28.085 = 28.085 H (hydrogen) | 16 | 61.5% | 1.008 | 16 × 1.008 = 16.128 m = 96.088 u + 15.999 u + 28.085 u + 16.128 u = 156.300 u Divide the mass for each element by m to calculate mass fractions. Then use the property that mass fractions must sum to one to check the work: | number of atoms | atom percent | mass fraction C (carbon) | 8 | 30.8% | 96.088/156.300 O (oxygen) | 1 | 3.85% | 15.999/156.300 Si (silicon) | 1 | 3.85% | 28.085/156.300 H (hydrogen) | 16 | 61.5% | 16.128/156.300 Check: 96.088/156.300 + 15.999/156.300 + 28.085/156.300 + 16.128/156.300 = 1 Compute mass percents using the mass fractions: Answer: | | | number of atoms | atom percent | mass percent C (carbon) | 8 | 30.8% | 96.088/156.300 × 100% = 61.48% O (oxygen) | 1 | 3.85% | 15.999/156.300 × 100% = 10.24% Si (silicon) | 1 | 3.85% | 28.085/156.300 × 100% = 17.97% H (hydrogen) | 16 | 61.5% | 16.128/156.300 × 100% = 10.32%

The first step in finding the oxidation states (or oxidation numbers) in [(1, 1-dimethyl-2-propynyl)oxy]trimethylsilane is to draw the structure diagram. Next set every oxidation number equal to the atom's formal charge: In [(1, 1-dimethyl-2-propynyl)oxy]trimethylsilane hydrogen is not bonded to a metal with lower electronegativity, so it will have an oxidation state of +1. Any element bonded to hydrogen gains the bonding electrons, decreasing their oxidation state by 1 for every bond: With hydrogen out of the way, look at the remaining bonds. There are 1 carbon-oxygen bond, 3 carbon-silicon bonds, 1 oxygen-silicon bond, and 4 carbon-carbon bonds. For each of these bonds, assign the bonding electrons to the most electronegative element. First examine the carbon-oxygen bond: element | electronegativity (Pauling scale) | C | 2.55 | O | 3.44 | | | Since oxygen is more electronegative than carbon, the electrons in this bond will go to oxygen. Decrease the oxidation number for oxygen (by 1 for single bonds, 2 for double bonds, and 3 for triple bonds), and increase the oxidation number for carbon accordingly: Next look at the carbon-silicon bonds: element | electronegativity (Pauling scale) | C | 2.55 | Si | 1.90 | | | Since carbon is more electronegative than silicon, the electrons in these bonds will go to carbon: Next look at the oxygen-silicon bond: element | electronegativity (Pauling scale) | O | 3.44 | Si | 1.90 | | | Since oxygen is more electronegative than silicon, the electrons in this bond will go to oxygen: Next look at the carbon-carbon bonds: element | electronegativity (Pauling scale) | C | 2.55 | C | 2.55 | | | Since these elements are the same the bonding electrons are shared equally, and there is no change to the oxidation states: Now summarize the results: Answer: | | oxidation state | element | count -4 | C (carbon) | 3 -3 | C (carbon) | 2 -2 | O (oxygen) | 1 -1 | C (carbon) | 1 0 | C (carbon) | 1 +1 | C (carbon) | 1 | H (hydrogen) | 16 +4 | Si (silicon) | 1

First draw the structure diagram for [(1, 1-dimethyl-2-propynyl)oxy]trimethylsilane, and for every non-hydrogen atom, count the σ-bonds. Note that double and triple bonds consist of one σ-bond together with one or two π-bonds: Identify those atoms with lone pairs: Find the steric number by adding the lone pair count to the number of σ-bonds: Consult the following chart to determine the hybridization from the steric number: steric number | hybridization 2 | sp 3 | sp^2 4 | sp^3 5 | dsp^3 6 | d^2sp^3 7 | d^3sp^3 Now assign the hybridization for each atom: Answer: | |

vertex count | 26 edge count | 25 Schultz index | 4666 Wiener index | 1294 Hosoya index | 23680 Balaban index | 7.101