Distinguish between polar bonds and polar molecules.
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which of the following molecules is polar? NO2 CO2 BF3 SF6 CCl4
convert (-sqrt2, -sqrt6) to polar coordinates with r > 0 and 0 ≤ θ < 2π.
Convert the rectangular coordinate (2,-2) to polar form and find two additional representations of this point. Can you check my work and explain how to finish the question? r=√(2)2+(-2)2 r=2√2 tan theta = (-2)/2 theta = -1 polar coordinate= (2√2, -1)
Write the polar equation in rectangular form. r = 12 sin theta Write the rectangular equation (x + 7)^2 + y^2 = 49 in polar form
Determine two pairs of polar coordinates for (3,-3) when 0°
I'm trying to find if potassium nitrate is polar or non-polar by using the electronegativity scale. Can someone check my work? Electronegativity: potassium: 0.82 nitrogen: 3.04 oxygen: 3.44 =3.44-3.04 =0.82-0.4 =0.4 =0.42 So the final answer is 0.42 and by
Which is more soluble in water? Briefly explain why. Acetic Acid: CH3CO(OH) OR Ethanol : CH3CH2OH I think its acetic acid because when observing its structure it is more polar than ethanol. And when using the like dissolves like rule, a more polar molecule
Hi. Is PO4(3-) polar or non-polar? Why or why not? Thanks! Look up the electronegativity of P and O. I think I remember that O is about 3.5 and P is about 2.1; therefore, each P-O bond is somewhat polar. Thus, the ion will be polar unless the Lewis
Sodium Chloride is the LEAST soluble in which of the following liquids? a. H2O b. CCl4 c. HF d. CH3OH e. CH3OOH I know NaCl is a polar molecule...and a dipole-dipole IMF bond? My guess is b because it's nonpolar and I think it's a London Dispersion IMF. Is
Chemistry (please check)
1)Which of the following compounds has the largest lattice energy: LiF LiCl NaF NaCl 2)Which of the following compounds has the most ionic character in its bonding: CaBr2 GeBr4 KBr GaBr3 3)Using the electronegativity table on page 364 of your text, which