Term
| Which ion(s) have the wrong charge? Na+, Mg+ or Al+ ? |
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Definition
| Mg+ should be Mg2+ and Al+ should be Al3+ Charges are at the top of the columns of the periodic table. |
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Term
| Ionic compounds are made of: |
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Definition
| positive ions and negative ions. |
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Term
| Ions form when neutral atoms gain or lose: |
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Definition
| electrons, in order to be like a noble gas. |
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Term
| Ionic compounds always start with a: |
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Definition
| metal, except for the one polyatomic NH4+1 |
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Term
| Which ion(s) have the wrong charge? Li-, O 2- , S2+ ? |
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Definition
| Li should be Li1+, and sulfur should be S2-. The charges are at the top of the periodic table. |
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Term
| Which of the following polyatomics is correct? NH+4, OH-1, PO3-2 ? |
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Definition
| OH-1 you may use the polyatomic chart on the test. |
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Term
| What does the suffix ‘-ate’ or ‘ite’ indicate in the name of the compound? |
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Definition
| that there is a polyatomic for the anion, and there are oxygens in the polyatomic. |
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Term
| hydrogen ions or also called hydronium ions |
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Definition
| What acids release into the water in which they are dissolved. |
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Term
| If an acid’s anion ends with ‘–ide’ such as |
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Definition
| The prefix ‘hydro’ is used in the acid name. |
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Term
| HCl(gas)= hydrogen chloride gas THEN: |
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Definition
| HCl(gas) in water causes the water to be called hydrochloric acid. |
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Term
| If a polyatomic is the anion of the acid, then: |
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Definition
| There’s NO prefix of ‘hydro’. |
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Term
| If an acid’s polyatomic ends with ‘-ate’ such as H2SO4 = hydrogen sulfate THEN: |
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Definition
The acid’s name ends with ‘-ic’.
hydrogen sulfate = H2SO4 = sulfuric acid |
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Term
| If an acid’s polyatomic ends with ‘ite’ such as H2SO3 = hydrogen sulfite THEN: |
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Definition
The acid’s name ends with ‘-ous’.
hydrogen sulfite = H2SO3 = sulfurous acid |
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Term
| Phosphoric acid is: Phosphorous acid is: |
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Definition
hydrogen phosphate = H3PO4= Phosphoric acid
hydrogen phosphite = H3PO3= Phosphorous acid |
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Term
| sour taste, electrolyte, litmus paper(pink), reacts with bases to make water and salt |
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Definition
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Term
| slippery, bitter taste, electrolyte, litmus paper(blue), reacts with acids to make water and salt |
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Definition
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Term
| 1+ is the charge of which acid ion? NH4 or H3O |
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Definition
H3O1+ is called ‘hydronium ion’ & is acidic.
NH41+ is called ‘ammonium ion’ and is a base. |
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Term
| If the hydrogen ion concentration is 1 x 10-9M then the solution is: |
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Definition
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Term
| If the hydrogen ion concentration is 1 x 10-4M, then the solution is: |
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Definition
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Term
| If the hydrogen ion concentration is 1 x 10-4M, then what is the hydroxide ion concentration? |
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Definition
| [OH-] = 1 x 10-10M and has a pH of 4. |
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Term
| If the hydroxide ion concentration is 1 x 10-6 M, then the hydrogen ion concentration is: |
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Definition
| [H+] = 1 x 10-8 M and has a pH of 8. |
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Term
| The symbol for ‘concentration’ is: |
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Definition
|
|
Term
| The concentration of hydronium ions in a neutral solution is: |
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Definition
| [H+] = 1 x 10-7 M and has a pH of 7. |
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Term
The formula for pH is: example,
hydronium concentration = [2.8 x 10-3M] |
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Definition
pH = -log [H ion] and would be keyed into the calculator as:
2.8 EE 3 ± log ± = 2.6 and would be acidic |
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Term
What is the pH of a solution that has a
hydronium concentration of 4.8 x 10-7M? |
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Definition
| 4.8 EE 7 ± log ± = 6.3 and would be acidic |
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Term
What is the pH of a solution that has a
hydronium concentration of 1.3 x 10-9M? |
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Definition
| 1.3 EE 9 ± log ± = 8.8 and would be basic |
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Term
| What is the pH of [10-11M]? |
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Definition
| 1 EE 11 ± log ± = 11 and would be basic |
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Term
| When the pH of a solution is between 0 and 6.99, the solution is: |
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Definition
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Term
| When the pH of a solution is between 7.1 and 14, the solution is: |
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Definition
|
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Term
| When the pH of a solution is exactly 7 the solution is: |
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Definition
|
|
Term
When the hydronium ion concentration is
1x10-7M. |
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Definition
|
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Term
| pH 3 is ten times _____ than pH 4 |
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Definition
| more concentrated, both are acids |
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Term
| pH 6 is ten times _____ than pH 5 |
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Definition
| more diluted, both are acids |
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Term
| pH 9 is ten times _____than pH 8 |
|
Definition
| more concentrated. both are bases |
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Term
| pH 8 is 100 times ______ than pH 10 |
|
Definition
| more diluted, both are bases |
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Term
|
Definition
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|
Term
|
Definition
| ionizes completely in water….example: HCl and H2SO4 |
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Term
|
Definition
| doesn’t ionize completely in water…some of the + and – ions won’t let go of each other….example: vinegar |
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Term
|
Definition
| ionizes completely in water….example: NaOH |
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Term
|
Definition
| doesn’t ionize completely in water…some of the + and – ions won’t let go of each other…..examples: NH4+ |
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Term
|
Definition
|
|
Term
| ionic compounds are always called: |
|
Definition
|
|
Term
| Acids start with a ________ that is acting like a metal. |
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Definition
|
|
Term
| Bases usually end with the polyatomic…. |
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Definition
|
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Term
|
Definition
| a way to figure the concentration of an acid or a base. |
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Term
|
Definition
| mixing an acid to a base to produce a salt and water. |
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Term
|
Definition
| a solution in which pH is kept relatively constant |
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Term
|
Definition
| have two hydrogens in front or two ionizable protons, such as H2SO4 |
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Term
|
Definition
| negative logarithm of the hydrogen ion concentration |
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|
Term
| acid theory…hydrogen-ion donor |
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Definition
| Bronsted-Lowry acid (medium theory) |
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|
Term
| acid theory…can accept an electron pair |
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Definition
| Lewis acid (hardest theory) |
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Term
| acid theory…dissociates into hydrogen ions |
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Definition
| Arrhenius acid (simplest theory) |
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Term
|
Definition
| have three hydrogens in front or three ionizable protons |
|
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Term
|
Definition
| has one hydrogen in front or one ionizable proton |
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Term
| Keeps the pH of a solution constant |
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Definition
|
|
Term
|
Definition
| summary of acid to base reaction |
|
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Term
|
Definition
| measuring instrument for titrations |
|
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Term
|
Definition
| phenolphthalein, pH paper, red cabbage juice, bromthymol blue, and several others. |
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Term
| How to find the products of an acid to base being combined: Example: HZ + ROH→ |
|
Definition
one product will be water…the result of the acid’s ‘H’
and the base’s ‘OH’.
The other product is the cation of the base
and the anion of the acid….RZ. |
|
|
Term
Correctly written skeleton equation for the acid to base reaction:
H2Z + R(OH)3 → |
|
Definition
H2Z + R(OH)3 → H2O + R2Z3…..
Where Z could be sulfate and R could be aluminum. |
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|
Term
Correctly written skeleton equation for the acid to base reaction:
H3Z + R(OH)2 → |
|
Definition
H3Z + R(OH)2 → H2O + R3Z2…..
Where Z could be phosphate and R could be magnesium. |
|
|
Term
Correctly written skeleton equation for the acid to base reaction:
H1Z + R(OH)1 → |
|
Definition
H1Z + R(OH)1 → H2O + R1Z1…..
Where Z could be chlorine and R could be sodium. |
|
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Term
| how to find the subscripts of a compound |
|
Definition
criss-cross the superscripts downward,
but don’t take the + or – downward. |
|
|
Term
| how to find the superscripts of a compound |
|
Definition
| look at the top of a periodic table and/or a polyatomic chart |
|
|
Term
how to balance a skeleton equation such as:
H3PO4 + Mg(OH)2 →
H2O + Mg3(PO4)2 |
|
Definition
-
Balance the Mg and (PO4) first.
-
Then count all the “H’s” on the left side of the arrow, then fix the “H’s” on the right side of the arrow.
-
Check to see if the “O’s” worked out on their own.
2H3PO4 + 3Mg(OH)2 →
6H2O + 1Mg3(PO4)2 |
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Term
| The coefficients of a balanced equation are also called: |
|
Definition
| moles of a balanced equation. |
|
|
Term
| another way to write 1x10-8M. |
|
Definition
|
|
Term
| hydronium ion symbols are: |
|
Definition
H3O+ or H3O+1 or H3O1+
[image] |
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|
Term
| What does the ‘M’ of 3M HCl mean? |
|
Definition
| The ‘M’ stands for ‘molar’ which tells how concentrated or diluted the HCl is. |
|
|
Term
| another way to write 1x10-6M |
|
Definition
|
|
Term
which number is bigger?
0.0001 or 0.001 |
|
Definition
|
|
Term
which number is bigger?
10-4 or 10-3 |
|
Definition
| 0.001 which is 10-3 is bigger than 0.0001 which is 10-4 |
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