Term
| Name the charge mass and role of protons, neutrons, and electrons. |
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Definition
Proton: +, 1 AMU, # of protons = atomic number
Electron: -, 1 AMU, # of protons = # of electrons in a stable atom
Nuetron: neutral, neglected, separates protons and stabilizes nucleus |
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Term
| Name the groups of the p-table. |
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Definition
Group A: Representative Elements
Group B: Transition Elements
Groups 1A-3A: Nonmetals are above stairs
Groups 4A- 7A: Metals
Group 8: Noble Gases
Below Stairs: Metaloids |
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Term
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Definition
Metal + Non-metal = Ionic Compound
Cation (+) is ALWAYS first, Anion (-) is ALWAYS second |
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Term
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Definition
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Term
| In respect to atomic radius; the ______ the charge the ______ the radius. |
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Definition
| The GREATER the charge, the SMALLER the radius |
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Term
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Definition
| Name FIRST as in p-table. Replace SECOND ending with -ide. When the first non-metal is NOT hydrogen...use mono, di, tri etc. |
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Term
| Where are type 1 metals in the p-table? |
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Definition
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Term
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Definition
Name FIRST as in p-table
Name SECOND with -ide ending |
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Term
| Naming a metal and polyatomic ion |
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Definition
Write metal as listed in p-table
Write ion as listed on chart |
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Term
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Definition
Name FIRST Metal as written in p-table.
Calculate charge of 1st metal and write it after in roman numerals.
Name SECOND with -ide ending. |
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Term
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Definition
if ending = -ate; stem + -ic
if ending = -ide; add HYDRO to beginning then stem + -ous
if ending = -ite; stem = -ous
Add ACID to the end |
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Term
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Definition
| 1 mole = atomic mass on ANY element |
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Term
| 1 mole = _________ atoms in ANY compound. |
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Definition
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Term
| What are the steps in finding the Empirical Formula? |
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Definition
1. Divide (% comp / atomic mass)
2. Divide all solutions by the SMALLEST solution yielded from step 1
3. If left with a fraction divide by multipliers. |
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Term
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Definition
0.5 multiply by 2!
0.33 or 0.66 multiply by 3! 0.25 or 0.75 multiply by 4!
0.2, 0.4, 0.6, 0.8 multiply by 5!
0.1 or 0.9 then ROUND! |
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Term
| What is the solute and solvent in respect to a solution? |
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Definition
Solute; the LOWER amount
Solvent; the HIGHER amount |
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Term
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Definition
| The amount of SOLUTE dissolved in a solution |
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Term
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Definition
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Term
To convert mL to L ____ by 1000
To convert kL to L ____ by 1000 |
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Definition
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Term
| The limiting reagent always yields the ____amount. |
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Definition
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Term
1 ATM relates to _______.
What does 1 ATM = ? |
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Definition
pressure
1 ATM = 760 torr
= 760 mm Hg
= 101.25 K pascal |
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Term
| As volume ________, pressure ________. |
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Definition
| As volume DECREASES, pressure INCREASES. |
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Term
When using Ideal Gas Law, what should the units be for:
PRESSURE
VOLUME
TEMPERATURE |
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Definition
Pressure - ATM
Volume - Liters
Temperature - Kelvin |
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Term
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Definition
0 + 273
or 0 degree Celsius + 273 |
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Term
| What does Standard Temperature Pressure (STP) mean? |
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Definition
Temperature = 273 Kelvin
Pressure = 1 ATM |
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Term
| What is the molar volume of any gas at STP? |
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Definition
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Term
| In a single displacement reaction the _____ active element replaces the _____ less active element. |
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Definition
| The MORE active element replaces the LESS active element. |
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Term
| A single displacement reaction can ONLY occur if... |
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Definition
| "A" is more active than "B" |
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Term
In a single displacement reaction;
_____ always comes before ______.
______ are always positive, while _____ are always negative.
Any element by itself = ? |
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Definition
METAL always comes before NON-METAL.
METALS are always positive, while NON-
METALS are always negative.
Any element by itself = 0. |
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Term
| What signifies a Double Displacement Reaction? |
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Definition
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Term
| When you do a double displacement reaction swap (__,__) and (__,__). |
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Definition
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Term
Steps to a double displacement reaction:
1)Write ________ product.
2)Write all the _______.
3)Write the ________ equation by _______ solid and ________ charges from that solid.
4)Write _______ equation by ________ and writing ________.
5)Remove ________. Then your left with the final equation, the ________ equation. |
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Definition
1) Write UNBALANCED product.
2) Write all CHARGES.
3) Write CHEMICAL equation by UNDERLINING solid & REMOVING it's charges.
4) Write the IONIC equation by BALANCING & writing CHARGES.
5) Remove CHARGES. The final equation is the NET-IONIC equation. |
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Term
| A neutralization reaction is a _______ ______ reaction, that ______ yields a ______. |
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Definition
| DOUBLE DISPLACEMENT reaction that ALWAYS yields a LIQUID. |
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Term
A combustion reaction ALWAYS produces the ____ product.
What product does it produce? |
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Definition
| ALWAYS produces CO2 + H2O |
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Term
| In a combustion reaction after balancing you have a fraction ______ the whole equation by the fractions ______. |
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Definition
| MULTIPLY the whole equation by the fractions DENOMINATOR. |
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Term
| Define Ionization Energy. |
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Definition
| Energy REQUIRED to move an electron from 1 atom to another. |
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Term
| As Ionization Energy ______ , ______ _____ _______. |
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Definition
| As Ionization Energy DECREASES, ATOMIC RADIUS DECREASES. |
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Term
| Non-metals are located _____ the _____. |
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Definition
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Term
| Transition metals have __ Valence shell(s); while Type 1 metals have __ valence shell(s). |
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Definition
Transition metals have 2 valence shells.
Type 1 metals have 1 valence shell. |
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Term
| Transition metals have __ Valence shell(s); while Type 1 metals have __ valence shell(s). |
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Definition
Transition metals have 2 valence shells.
Type 1 metals have 1 valence shell. |
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Term
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Definition
| Resemble metals but are NON-METALS. |
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Term
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Definition
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Term
| In order to become stable, METALS try to ______ valence electrons and become stable _____. |
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Definition
| LOOSE electrons and become stable CATIONS. |
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Term
| In order to become stable, NON-METALS try to _____ valence electrons and become stable _____. |
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Definition
| GAIN electrons and become stable ANIONS. |
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Term
1)Sub-level S has ___ box(es)& __ electron(s)
2)Sub-level P has ___ box(es)& __ electron(s)
3)Sub-level D has ___ box(es)& __ electron(s)
4)Sub-level F has ___ box(es)& __ electron(s) |
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Definition
S: 1 Box, 2 Electrons
P: 3 Boxes, 6 Electrons
D: 5 Boxed, 10 Electrons
F: 7 boxes, 14 Electrons |
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Term
| With respect to the sub-level box diagram what element MIGRATES? |
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Definition
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Term
| Sub-level f has _____ energy and appears in the _____ energy level. |
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Definition
| HIGH energy, appears in 6th level |
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Term
Principle Quantum #'s
What are they and where do they appear? |
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Definition
1,2,3,4,5,6,7
Top of Boxes |
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Term
Secondary Quantum #'s
What are they and where do they appear? |
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Definition
S = 0
P = 1
D = 2
F = 3
Top of Boxes |
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Term
Magnetic Quantum #'s
What are they and where do they appear? |
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Definition
-...0...+
#'s 1-7
They go under each box with the ZERO UNDER THE CENTER BOX
Negatives are on the left side of the 0, positives on the right |
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Term
Spin Quantum #'s
What are they and where do they appear? |
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Definition
-1/2 and +1/2
If the last arrow is facing UP it is +1/2
If Last arrow is facing DOWN it is -1/2 |
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Term
Periodic Properties
Group(s) 1A, 2A, all B group, above stairs, below stairs, Group 7, and Group 8. |
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Definition
1A: Alkaline Metals
2A: Alkaline Earth Metals
ALL B: Transition Metals
Above Stairs: Non-metals
Below Stairs: Metaloids
7: Halogens
8: Noble Gases |
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Term
Atomic Radius Table
Start in ____ _____ corner, read _____ to _____
Top Right = _______ _____
_______ = Largest Radius |
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Definition
Start at TOP RIGHT CORNER, read RIGHT to LEFT.
Top Right = SMALLEST RADIUS
BOTTOM LEFT = Largest Radius |
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Term
| On the product side of a Single Displacement Reaction for the compound, the charge of one becomes ______ of the other and vice versa. |
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Definition
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