- 18.104.22.168.28: What is ionization energy?
- 22.214.171.124.29: Why is measuring the size of an atom difficult?
- 126.96.36.199.30: What can you tell about an atom that has high electronegativity?
- 188.8.131.52.31: How does electron shielding affect atomic size as you move down a g...
- 184.108.40.206.32: What periodic trends exist for ionization energy?
- 220.127.116.11.33: Describe one way in which atomic radius is defined.
- 18.104.22.168.34: Explain how the trends in melting and boiling points differ from th...
- 22.214.171.124.35: Why do both atomic size and ionic size increase as you move down a ...
- 126.96.36.199.36: How is electron affinity different from electronegativity?
- 188.8.131.52.37: What periodic trends exist for electronegativity?
- 184.108.40.206.38: Why is electron shielding not a factor when you examine a trend acr...
- 220.127.116.11.39: Explain why the noble gases have high ionization energies.
- 18.104.22.168.40: What do you think happens to the size of an atom when the atom lose...
- 22.214.171.124.41: With the exception of the noble gases, why is an element with a hig...
- 126.96.36.199.42: Explain why atomic radius remains almost unchanged as you move thro...
- 188.8.131.52.43: Helium and hydrogen have almost the same atomic size, yet the ioniz...
- 184.108.40.206.44: Why does mercury, Hg, have such a low melting point? How would you ...
- 220.127.116.11.45: What exceptions are there in the increase of ionization energies ac...
Solutions for Chapter 4.3: Trends in the Periodic Table
Full solutions for Modern Chemistry: Student Edition 2006 | 1st Edition
An OR group.
When applying Woodward-Fieser rules, the groups attached to the chromophore.
A neutral molecule with nonadjacent positive and negative charges. An example of a betaine is the intermediate formed by addition of a Wittig reagent to an aldehyde or ketone
Valence electrons involved in forming a covalent bond (i.e., shared electrons).
A positively charged, bridged intermediate formed during the addition reaction that occurs when an alkene is treated with molecular bromine (Br2).
A species in which a carbon atom has only six electrons in its valence shell and bears a positive charge
A force that becomes significant when polar molecules come in close contact with one another. The force is attractive when the positive end of one polar molecule approaches the negative end of another. (Section 11.2)
A catalyst that is in a different phase from that of the reactant substances. (Section 14.7)
Any b-elimination that occurs preferentially to give the less substituted alkene as the major product.
In nomenclature, a numberused to identify the location of a substituent.
net ionic equation
A chemical equation for a solution reaction in which soluble strong electrolytes are written as ions and spectator ions are omitted. (Section 4.2)
An electrophilic aromatic substitution reaction that involves the installation of a nitro group (NO2) on an aromatic ring.
A system for naming organic compounds.
When used in the context of fats and oils, a mixture of triglycerides that is liquid at room temperature
The pressure that must be applied to a solution to stop osmosis from pure solvent into the solution. (Section 13.5)
An intermediate that is believed to be formed during Wittig reactions.
A compound with the structure R2CRN!OH.
The conjugate base of phenol or a substituted phenol.
A polymer containing the !NHCO2! group as a repeating unit
Tertiary structure of proteins
The three-dimensional arrangement in space of all atoms in a single polypeptide chain.
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