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(a)
Interpretation:
The formulas for
Concept introduction:
The general rules for writing the common names of compounds of metals that form more than one ion are:
1) The root name of the metal is followed by the suffix
2)The root name of the metal is followed by the suffix
For writing the systematic name of the compound, a roman numeral within parentheses is written immediately after the name of the metal ion to indicate the charge on it.
(b)
Interpretation:
The formulas for lithium nitride, lithium nitrite, and lithium nitrate are to be determined.
Concept introduction:
The general rules for naming ionic compounds are as follows:
1) In ionic compounds, the cations are named before the anions.
2) In binary ionic compounds, the name of the cation is the same as the name of the metal. The name of the anion includes the root name of the non-metal and a suffix
3) In polyatomic ions in which a non-metal is bonded to one or more oxygen atoms. In two oxoanions in the family, the ion with fewer oxygen atoms has the non-metal root name and a suffix
(c)
Interpretation:
The formulas for strontium hydride and strontium hydroxide are to be determined.
Concept introduction:
The general rules for naming ionic compounds are as follows:
1) In ionic compounds, the cations are named before the anions.
2) In binary ionic compounds, the name of the cation is the same as the name of the metal. The name of the anion includes the root name of the non-metal and a suffix
(d)
Interpretation:
The formulas for magnesium oxide and
Concept introduction:
The general rules for writing the common names of compounds of metals that form more than one ion are:
1) The root name of the metal is followed by the suffix
2)The root name of the metal is followed by the suffix
For writing the systematic name of the compound, a roman numeral within parentheses is written immediately after the name of the metal ion to indicate the charge on it.
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Chapter 2 Solutions
Chemistry: The Molecular Nature of Matter and Change - Standalone book
- Nonearrow_forwardIn the solid state, oxalic acid occurs as a dihydrate with the formula H2C2O4 C+2H2O. Use this formula to calculate the formula weight of oxalic acid. Use the calculated formula weight and the number of moles (0.00504mol) of oxalic acid in each titrated unknown sample recorded in Table 6.4 to calculate the number of grams of pure oxalic acid dihydrate contained in each titrated unknown sample.arrow_forward1. Consider a pair of elements with 2p and 4p valence orbitals (e.g., N and Se). Draw their (2p and 4p AO's) radial probability plots, and sketch their angular profiles. Then, consider these orbitals from the two atoms forming a homonuclear л-bond. Which element would have a stronger bond, and why? (4 points)arrow_forward
- Write the reaction and show the mechanism of the reaction. Include the mechanism for formation of the NO2+ 2. Explain, using resonance structures, why the meta isomer is formed. Draw possible resonance structures for ortho, meta and para.arrow_forwardNonearrow_forward3. A molecular form of "dicarbon", C2, can be generated in gas phase. Its bond dissociation energy has been determined at 599 kJ/mol. Use molecular orbital theory to explain why energy of dissociation for C₂+ is 513 kJ/mol, and that for C2² is 818 kJ/mol. (10 points)arrow_forward
- 9.73 g of lead(IV) chloride contains enough Cl- ions to make ____ g of magnesium chloride.arrow_forward6. a) C2's. Phosphorus pentafluoride PF5 belongs to D3h symmetry group. Draw the structure of the molecule, identify principal axis of rotation and perpendicular (4 points) b) assume that the principal axis of rotation is aligned with z axis, assign symmetry labels (such as a1, b2, etc.) to the following atomic orbitals of the P atom. (character table for this group is included in the Supplemental material). 3s 3pz (6 points) 3dz²arrow_forward2. Construct Lewis-dot structures, and draw VESPR models for the ions listed below. a) SiF5 (4 points) b) IOF4 (4 points)arrow_forward
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