Answer:
O₃
Explanation:
Consider the molecule CO₂. The carbon is sp hybridized. Carbon has 4 valence electrons and oxygen contributes 2 electrons, 1 for each C=O which indicates that there are 8 electrons around the carbon. Since there are 4 bonds all of them are bond pairs. Each C=O double bond uses 2 bond pairs which are considered as single unit. These two double bond units try to get as far apart as possible making the molecule adopt a linear geometry.
Considering the H₂S molecule both oxygen and sulfur are the in the same group, which means both have a valence of 6. The four valence orbitals of sulfur, one 1 s orbital and three 3p orbitals mix together and forms four sp³ hybridized orbitals. Of the four hybridized orbitals, two overlaps with the 1s orbital of hydrogen forming 2 (S - H) bonds while the other two sp³ orbitals remain on sulfur which has lone pair of electrons. Because of the presence of lone pair, the angle between H-S-H bond is slightly less than the ideal tetrahedral bond angle. Thus, H2S having 2 bonding electron pair and 2 lone pairs has a bent shape.
Considering O₃ and according to the VSEPR theory ozone molecule must have a trigonal – planar geometry. It has a total of 18 valence electrons. From the resonance structure given below it is clear the 4 pairs of electrons exit as bonding pair, sp² or σ- bond and the remaining 10 electrons exit as lone pair. Of the three un- hybridized p orbitals one is anti – bonding and remains empty. In ozone the π bond is distributed between the two bonds, and each receives half a π bond. For this molecule the electron pair geometry is trigonal planar but the molecular geometry is bent. The presence of lone pair exerts slight repulsion on the bonding oxygen atoms and a slight compression of the bond angle greater than 120°.
In carbonate ion, <u>the carbon is sp² hybridized</u>. The carbon has 4 valence electrons and there are four bonds to the oxygen which add another 4 making a total of 8. There are 4 pairs of bonding electrons and no lone pair. Of the 4 bond pairs, 2 pairs are used in forming double bond C=O and 2 bond pairs in forming the two C-O single bonds., Thus CO₃²⁻ adopts a trigonal planar geometry.
Of the two molecules only ozone and carbonate ion, have sp2 hybridized central atoms. In ozone the central atoms have lone pair of electrons the hybridization around is sp². Hence the correct option is O₃
Answer:
C and D
Explanation:
Atoms with five, six or seven valance electrons gain electrons to complete the octet because it is more convenient for the atoms to gain three, two or one electron as compared to lose five, six or seven electrons. Thus atoms with five, six or seven valance electrons form negative ions by gaining electrons.
Atoms with one, two or three valance electrons lose the electrons to get complete octet because it is more convenient for the atoms to lose one two or three electrons as compared to gain the seven, six or five electrons. The atoms with one, two or three valance electrons form positive ions.
Answer:
22.13g
Explanation:
We'll begin by writing a balanced equation for the reaction. This is illustrated below:
2C2H2 + 5O2 —> 4CO2 + 2H2O
Next, we'll calculate the mass of C2H2 and O2 that reacted from the balanced equation. This is illustrated below:
Molar Mass of C2H2 = (12x2) + (2x1)
= 24 + 2 = 26g/mol
Mass of C2H2 that reacted from the balanced equation = 2 x 26 = 52g
Molar Mass of O2 = 16x2 = 32g/mol
Mass of O2 that reacted from the balanced equation = 5 x 32 = 160g
Now, we can obtain the mass of C2H2 that will react with 68.1g of O2 as follow:
From the balanced equation above,
52g of C2H2 reacted with 160g of O2.
Therefore, Xg of C2H2 will react with 68.1g of O2 i.e
Xg of C2H2 = (52x68.1)/160
Xg of C2H2 = 22.13g
Therefore, 22.13g of C2H2 is needed to react with 68.1g of O2
With every electron stationed in its own orbital or paired off with each other in the higher energy level, the energy level is balanced and stable. The atoms that utilize this exception are Molybdenum, Chromium, Gold, Silver, and Copper.
Answer:
i know 3, reproduction, organisms, and variations in traits
Explanation:
