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The pH of an aqueous solution of the salt NH₄C₂H₃O₂ (ammonium acetate) will _________.

a) be basic (because it is a weak acid-strong base salt)

b) be acidic (because it is a strong acid-weak base salt)

c) be neutral (because it is a strong acid-strong base salt)

d) not be known (because it is a weak acid-weak base salt)

e) no correct response

For Each of the following dissolved in water, identify if the solution is strong acid, weak acid, strong base, weak base, or has no effect on pH.

a. HBr

b. KCl

c. FeCl₃

_d. Na₃PO₄

e. NH₃

f. Sodium acetate

g. NaF

15.7) Which of the following is correctly identified? a. NH3, strong acid b. NaOH, strong base c. HCl, weak acid d. H2CO3, strong acid e. Ca(OH)2, weak base

_____ 1. An element has how many classes of properties to describe it? a. 1 b. 2 c. 3 d. 4 ______

2. When copper turns green, it is an example of its a. chemical property c. value b. physical property d. thickness _____

3. A chemical experiment is a. never done in the laboratory b. a carefully controlled and measured testing of a sample’s properties c. something to try once and then move on to other things d. always performed at room temperature _____

4. Which of the following is not a property of gold? a. it is highly reactive c. it is naturally found as a solid b. it melts at 300C d. it has luster _____

5. The chemical shorthand name for molybdenum is a. Mo b. Mb c. Md d. Mn _____

6. Milli is the prefix used to show a. 106 b. 107 c. 10-3 d. 10-1 _____

7. Protons share the dense nucleus with a. nuetrons b. molecules c. electrons d. atoms ______

8. Electrons are a. sub-atomic particles with a +1 charge b. equal to the number of protons in a nucleus c. said to be charmed d. sub-atomic particles with a +2 charge _____

9. The force that binds 2 or more atoms together is known as a. a chemical bond b. valence c. joules d. electromagnetsm ______

10. A molecular formula a. gives the total number of moles in a compound b. is used only in derived chemical formulas c. gives the number of each elemental atom in a molecule d. is handy to have, but doesn’t include all the elements _____

11. The neutron is a subatomic a. with no electric charge b. with a -1 electric charge d. with no counterpart within the atom. _____

12. The Aufbau principle a. defines the undefined particles of the nucleus b. is a method used to describe an atom’s ground state c. provides radioactive levels of elements d. lists the negative and positive spin of atoms _____

13. Ionization energy of an element a. is the amount thrust needed to fly at mach speed b. is the energy a neutron generates c. cannot be calculated or observed d. is the energy needed to remove an electron from an atom _____

14. Noble gases a. are highly reactive with helium b. are highly reactive with strontium c. are unreactive under normal condition d. are related to nobility ____

15. A bond between atoms in a molecule is a. made up of a shared electron pair b. stronger than static electricity c. always located in the 3s orbital d. only a double bond ____

16. Elements in 1V of the periodic table have a. 3 valence electrons c. 5 valence electrons b. 4 valence electrons d. 6 valence electrons _____

17. The electron configuration of an atom a. is determined by the amount of kinetic energy present b. is found by calculating atomic mass c. is written as s,p,d,f subshells d. describes the specific distribution of electrons in a subshell ____

18. The Pauli exclusion principle states that a. any atom with a free s orbital can form bonds b. no two atoms can occupy the same orbital unless their spins are different c. 2 atoms sharing an orbital are matched exactly d. atoms of the same configuration do not change _____

19. In water molecules, how many oxygen atom(s) combine with hydrogen atoms? a. 1 b. 2 c. 3 d. 4 ______

20. Reduction is the process a. calculating the oxidation number of oxygen b. increasing the oxidation number ok oxygen c. losing hydrogen or electrons in a reaction d. gaining hydrogen or electrons in a reaction

Does the octet rule mean that a diatomic molecule has 16 valenceelectrons? Select from the following:

A. Yes, each atom has 8 valence electrons. Two atoms, with 8electrons each, is 16 valence electrons.

B. No, the octet rule means there are always 8 valence electronsand only 8 valence electrons.

C. Most of the time there are 16 valence electrons, but thereare exceptions to the octet rule (odd-electron species, expandedoctets, etc.) that could make it more or less than 16.

D. No, the octet rule means there are 8 valence electrons aroundeach atom, but bonding electrons get counted for the atoms on bothsides of the bond, so there are normally fewer than 16 valenceelectrons unless there is an expanded octet.

1.) How is the number of valence electrons in an atom related to its tendency to gain or lose electrons during compound formation?

Atoms with or ---Select--- (more ,fewer )valence electrons tend to lose them; atoms with or ---Select--- (more, fewer) valence electrons tend to gain more electrons.

2.) Explain the process in which one atom of sodium bonds with one atom of chlorine. (Type your answer using the format 1+ and 2-.)

Sodium bonds with chlorine via an ionic bond. ---Select---( Sodium ,Chlorine) will lose its valence electron to form a ---Select--- (sodium ,chloride) ion with a charge of _______ that has a stable shell (octet) of electrons. This extra electron is used by a ---Select--- (sodium, chlorine )atom to form a stable ---Select---( sodium ,chloride ) ion with a charge of _______. Electrical forces attract these ions together to form a strong, ionic bond.

The formula for acetone is CH3COCH3. In acetone, the second carbon atom is bonded to the oxygen atom and to both of the other carbon atoms. Draw acetone's Lewis diagram and use the table above to estimate its bond lengths.

(C-C): 1.54Ã

(C=C): 1.34Ã

(C=O): 1.20Ã

(C-H): 1.10Ã

Carbon-Carbon: ___________________Ã

Carbon-Oxygen: _________________Ã

(With Steps Please)

Please help with 2 and 3!!!!!!

Any help/explanation would be greatly appreciated. Thank you!

which c-c-c bond angle in the molecule would be approximately 120°

Some cleansers contain brominated salts as the oxidizing agents. The bromate ion, BrO3^- , oxidizes the iodide ion as follows:
BrO3^- + 6I^- + 6H^+ → 3I2 +Br^- + 3H2O
On a molecular basis, which is a more effective bleaching agent, KBrO3 or NaOCl? Explain.

Some cleansers contain bromate salts as the oxidizing agent. The bromate ion, BrO,-, oxidizes the iodide
ion as follows:
BrO, + 61- + 6H* ->3L + Br + 34,0
On a molar basis, which is a more effective bleaching agent, KBrO, or NaOCI?

Saludos, favor ayuda con esto!