CHEM103 / CHEM 103 Module 3: (Latest Update
) General Chemistry I with Lab |
Questions & Answers | Grade A | 100% Correct.
Portage Learning
1. Physical properties of ionic compounds: Solid w crystalline structure,
hard/brittle, high melting and boiling points, not electrically conductive
when solid but are when molten/dissolved, water soluble, metal and
nonmetal
2. Binary compound: a compound composed of two elements
3. Group 1 (alkali metals) cation charge?: 1+
4. Group 2 (alkaline earth metals) cation charge?: 2+
5. Post transition metal with fixed charge?: aluminum
6. Isoelectronic: 2 elements with the same number of electrons/configuration
7. Aluminum (group 13) cation charge?: 3+
8. Post Transition Metals: the metals on the left side of the staircase after
transition metals
,9. How do post transition metals ionize?: Can form ions of (group #) - 10,
most are variable charge except aluminum
10. Which categories can form variable charges?: Transition, post-
transition, inner transition
11. How do most nonmetals ionize?: They gain enough electrons to match
nearest noble gas
12. Halogens anion charge?: 113. Chalcogens anion charge?: 214.
Pnictogens anion charge?: 3-
15. Covalent Bonds: attractive force between the nucleus of a molecules
atoms and pairs of electrons between the two atoms, shared electrons
16. Covalent compound: a chemical compound formed by the sharing of
electrons 17. Physical properties of covalent compounds: Typically liquid or
gas under normal conditions, if solid, usually soft, with low melting/boiling
points, poor conductors, usually not soluble in water, often two nonmetals
18. Why are covalent compounds usually not water soluble?: Water is polar
and usually is easier to dissolve charged substances
, 19. Is covalent bonding endo or exothermic?: Exothermic because bonding
stabilizes the atoms more, so energy is released, and a bond forms when the
energy bottoms out (breaking the bond is endothermic)
20. Bond Length: the average distance between the nuclei of two bonded
atoms
(distance at which lowest potential energy is achieved)
21. Pure covalent bond: bond between two atoms of the same/similar
electronegativities in which electrons are equally shared (aka nonpolar)
22. Electron density: probability that an electron will be found in a particular
area of an atom
23. Polar covalent bond: Bond formed between atoms w/ different
electronegativity, electrons more attracted to one atom than other and are
not shared equally
24 Partial charge: In a polar covalent bond, charge on one side of the
molecule that is partial negative on more electronegative side and partial
positive on less electronegative side
) General Chemistry I with Lab |
Questions & Answers | Grade A | 100% Correct.
Portage Learning
1. Physical properties of ionic compounds: Solid w crystalline structure,
hard/brittle, high melting and boiling points, not electrically conductive
when solid but are when molten/dissolved, water soluble, metal and
nonmetal
2. Binary compound: a compound composed of two elements
3. Group 1 (alkali metals) cation charge?: 1+
4. Group 2 (alkaline earth metals) cation charge?: 2+
5. Post transition metal with fixed charge?: aluminum
6. Isoelectronic: 2 elements with the same number of electrons/configuration
7. Aluminum (group 13) cation charge?: 3+
8. Post Transition Metals: the metals on the left side of the staircase after
transition metals
,9. How do post transition metals ionize?: Can form ions of (group #) - 10,
most are variable charge except aluminum
10. Which categories can form variable charges?: Transition, post-
transition, inner transition
11. How do most nonmetals ionize?: They gain enough electrons to match
nearest noble gas
12. Halogens anion charge?: 113. Chalcogens anion charge?: 214.
Pnictogens anion charge?: 3-
15. Covalent Bonds: attractive force between the nucleus of a molecules
atoms and pairs of electrons between the two atoms, shared electrons
16. Covalent compound: a chemical compound formed by the sharing of
electrons 17. Physical properties of covalent compounds: Typically liquid or
gas under normal conditions, if solid, usually soft, with low melting/boiling
points, poor conductors, usually not soluble in water, often two nonmetals
18. Why are covalent compounds usually not water soluble?: Water is polar
and usually is easier to dissolve charged substances
, 19. Is covalent bonding endo or exothermic?: Exothermic because bonding
stabilizes the atoms more, so energy is released, and a bond forms when the
energy bottoms out (breaking the bond is endothermic)
20. Bond Length: the average distance between the nuclei of two bonded
atoms
(distance at which lowest potential energy is achieved)
21. Pure covalent bond: bond between two atoms of the same/similar
electronegativities in which electrons are equally shared (aka nonpolar)
22. Electron density: probability that an electron will be found in a particular
area of an atom
23. Polar covalent bond: Bond formed between atoms w/ different
electronegativity, electrons more attracted to one atom than other and are
not shared equally
24 Partial charge: In a polar covalent bond, charge on one side of the
molecule that is partial negative on more electronegative side and partial
positive on less electronegative side
