The smaller dipole moment in CO , the reason to be predicted. Concept Introduction : Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dots. Formal charge: The charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, regardless its relative electronegativity. Ionic bond: The electrostatic force of attraction between two oppositely charged ions result in ionic bonding. Covalent bond: The equal sharing of two electrons between two atoms (identical atoms or nearly close electronegativity values) in a compound.

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mical lation or mula trations, AAAAAAAAAAAAA Experiment #8 Electrical conductivity & Electrolytes Conductivity of solutions FLINN Scientific conductivity meter scale - RED LED Scale 0 Green LED OFF OFF 1 Dim OFF 2 medium OFF Bright Dim 4 Very Bright Medium 3 LED Conductivity Low or None' Low Medium High very high SE = Strong Electrolyte, FE = Fair Electrolyte WE Weak Electrolyte, NE= Noni Electrolyte 9 0.1 M NaOH. 10. 0.1M NH3 11. D.1M HCT 12. 0.1 M HC2H3D2 13 0 m H2SO4 Prediction observed conductivity ? Very bright red, dim green (4) ? Saturated Bright red, dim green 3 Cacal) Bright red, dim green 3 Prediction Bright red, No green ? observed Bright red,dim green ? Conductivity Just red? I Can you help me understand how I'm supposed to find the predictions of the following solutions? I know this is an Ionic compound and that the more ions in a solution means it is able to carry a charge, right? AAAAAA The light are not matching up with the scale So I'm confused about what I should be…

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Chapter 8, Problem 29Q

Interpretation Introduction

Interpretation:

The smaller dipole moment in CO, the reason to be predicted.

Concept Introduction:

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dots.

Formal charge: The charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, regardless its relative electronegativity.

Ionic bond: The electrostatic force of attraction between two oppositely charged ions result in ionic bonding.

Covalent bond: The equal sharing of two electrons between two atoms (identical atoms or nearly close electronegativity values) in a compound.

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