CHEMISTRY COMMUNITY

Mark 1D

Cations lose electrons, giving a positive charge

Mark 1D

Bronsted base because H- is a proton acceptor

Mark 1D

Lewis acids are defined as accepting a pair of electrons whilst the Lewis bases are donors of electrons. So it would be based on whether the molecule accepts or gives electron pairs

Mark 1D

I do not think there are exceptions to the electronegativity trend which goes up and to the right on the periodic table

Mark 1D

because d orbitals allow those elements to have expanded octets so hybridization can show the d along with the s and p orbitals due to the large amount of valence electrons

Mark 1D

Lewis describes lewis acid as an acceptor of a lone pair of electrons whilst Bronstead describes an acid as a donor of a proton

Mark 1D

The elements in the d block can violate the octet rule because of the presence of the d orbital into which more electrons can reside

Mark 1D

Sigma bonds overlap more than pi bonds, allowing for more strength whilst also allowing for rotation

Mark 1D

Smaller atomic radius cations have more polarizing power. A higher charge also gives more polarizing power

Mark 1D

elements in the d block are exceptions as they are able to fill their d orbital with more electrons, allowing for an expanded octet

Mark 1D

I believe oxygen is more electronegative as it is higher than chlorine on the periodic table

Mark 1D

a single bond corresponds to a sigma bond, whilst a double bond is 1 sigma and 1 pi and a triple bond is 1 sigma and 2 pis

Mark 1D

p shell has 3 orbitals I believe

Mark 1D

3X10^8 should be fine I think

Mark 1D

Can someone explain the solution for 2F.1 in the 7th Edition? "State the relative orientation of each of the following hybrid orbitals: (a)sp^3; (b) sp; (c)sp^3d^2; (d) sp^2.

Mark 1D

electrons fill up the s and p orbital. once those orbitals are filled, d orbital is needed for an atom to have more than 8 valence electrons

Mark 1D

Howdy partners. What is the reasoning for why double bonds are shorter (and therefore stronger) than single bonds? Thanks

Mark 1D

Howdy. Can one of ya'll explain how having a greater number of orbitals, such as a d orbital, allow an element to have an expanded octet? Thanks.

Mark 1D

Howdy ya'll. Can someone explain why the ground state electron configuration for Ag^+ is [Kr]4d^10 in question 2A.21? Thanks

Mark 1D

Howdy! 2A.6 asks for the ground-state electron configuration of the ion P^3-. Can someone explain how I would go about solving this?

Mark 1D

Howdy partners. Are ionic bonds always between non-metals and metals?

Mark 1D

Howdy there. I was wondering about the conceptual explanation behind why higher orbitals have more energy. Is it because of distance from the positively charged nucleus?

Mark 1D

Howdy! 1B.27 says "A bowling ball of masss 8.00 kg is rolled down a bowling alley lane at 5.00 +/ 5.0 m/s. What is the minimum uncertainty in its position?" Can one of ya'll explain to me how I use the uncertainty equation to obtain the minimum uncertainty?

Mark 1D

Howdy ya'll. 1B.25 states "What is the minimum uncertainty in the speed of an electron confined within a lead atom of diameter 350 pm? Can somebody explain how to obtain the solution please. Thanks

Mark 1D

A single photon requires the sufficient energy needed to remove a single electron. :)

Mark 1D

Does anybody know how long a wavelength must be to be "measurable"?

Mark 1D

1A.3 Which of the following happens when the frequency of electromagnetic radiation decreases? Explain your reasoning. (c) The extent of the change in the electrical field at a given point decreases. Can someone explain what happens to the "extent of the change in the electrical field at a give...

Mark 1D

The molar mass of the metal hydroxide M(OH)2 is 74.10 gmol. What is the molar mass of the sulfide of this metal? I understand how to obtain molar mass but how do I identify the sulfide of M(OH)2? Thanks

Mark 1D

When working on the answer to a question, does anybody know if we have to show units in our work? I understand our final answer must have units.

Mark 1D

I believe atomic weight is the measured weight of the atom whilst the molecular weight is the measured weight of the molecule (so add weights of the atoms within the molecule). ;)

CHEMISTRY COMMUNITY

Search found 30 matches

Re: ions

Re: H-

Re: Lewis Acids & Bases

Re: Exceptions

Re: Expanded Octet Hybridizations

Re: Lewis v Bronsted

Re: Elements that break the octet rule

Re: pi vs sigma

Re: Polarizing Power: Size vs. Charge

Re: Exceptions

Re: Ionic Character

Re: Number of sigma and pi bonds

Re: Orbitals

Re: Speed of light

2F.1 7th Edition

Re: Octet Expansion

Why Are Double Bonds Shorter

Understanding Expanded Octets

2A.21 7th Edition Question

2A.6 7th Edition

Question regarding ionic bonds

Concept Behind Orbitals

HW Question Regarding 1B.27

1B. 25 7th Edition

Re: Photons

Measurable Wavelengths

1A.3 7th Edition Question

E15 7th Edition

Question regarding showing units within work

Re: Atomic Weight vs Molecular Weight