-
How many sig figs in 0.0300?
3
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How many sig figs in 1600km?
2
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6.3 cm X 2.5 cm = ?
19 cm2
-
-
What is vol of block: 2.0cm by 3.0cm by 4.0cm?
24 cm cubed
-
What is the mass of 19 mL of Al (density = 2.7 g/cm3)?
51g
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92mL is the same as (92L, 92 cubic cm, 92 cm or 0.092 cubic cm)?
92 cubic cm
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Which of these is a homogeneous mixture? a)milk b)water c)NaCl d)Norm Saline
Normal Saline
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Which of these is a chemical change? a) breaking glass b)cutting grass c)frying an egg
Frying an egg
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Which particle of an atom has no charge?
Neutron
-
The number of neutrons in ¹⁷₈O²⁻ ion is ____
9
-
Which type of electron magnetic radiation has the most energy - blue light / UV light / red light / infared light?
UV light
-
Different isotopes of the SAME element have different a) # of p+ & e- b) masses & #s of n c)#s of p+ & n d) masses & #s of p+)?
Masses & Numbers of Neutrons
-
To be an atom or ion of magnesium there MUST be ____ protons.
12
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When an atom of copper is heated and a blue color is seen (A) its p+ jump to higher energy levels & return to lower levels (B) its n jump to higher energy levels & return to lower levels (C) its e- jump to higher energy levels & return to lower levels
Its e- jump to higher energy levels & return to lower levels
-
Which element is found in fluorescent light bulbs?
Mercury
-
For the element sulfur (S) there are how many valence electrons?
6
-
The element sulfur will most likely form an ion with what charge?
-2
-
When an atom of sulfur forms an ion it will be isoelectronic with ____.
Ar
-
Cl, Ne, O, or Ar will have the same # of valence e⁻ as sulfur.
O
-
Kr, K, Ba or Br is a noble gas.
Kr
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Which of these elements has the biggest atoms: Na, Cl or Rb?
Rb
-
Which of these elements has the greatest electronegativity: Na, Cl or Rb?
Cl
-
For atoms of elements, in general, the smaller the atom the ______ the electronegativity.
Larger
-
Which of these will have the e⁻ config 1s² 2s² 2p⁶? (A) Ne (B) F¹⁻ (C) Na¹⁺ (D) all of these
All of these
-
What is std scientific notation for 75,000?
7.5x10⁴
-
What is std scientific notation for 0.04090?
4.090x10⁻²
-
What is the formula for the density of an object?
d=m/v
-
What is the formula for specific gravity?
SG= d of object / d of H₂O
-
-
-
Calculate the atomic mass of naturally occurring Cl if 75.77% of Cl atoms are Chlorine-35 (mass of 35.00) & 24.23% is Chlorine-37 (mass of 37.00).
35.49 amu
-
-
-
An atom of ¹⁵₇N has how many protons? Neutrons? Electrons? Atomic #? Mass #?
- 7 p⁺
- 7e⁻
- 8n
- Atomic # = 7
- Mass # = 15
-
What is the formula for Calcium Hydroxide?
Ca(OH)₂
-
What is precision?
Degree of agreement between repeated measurements
-
What is accuracy?
How close you are to the right answer
-
What is a heterogeneous mixture?
-
What is ionization energy?
Energy needed to remove an electron fr an isolated atom
-
Describe electron affinity.
Energy released when a single e⁻ is added to an isolated atom
-
As you go down a grp electronegativity ____.
Decreases
-
As you read across a period electronegativity _____.
Increases
-
Affinity ______ as you go down a grp.
Decreases
-
Affinity ____ as you go across a period.
Increases
-
Atomic size increases going from ____ to ____.
top to bottom
-
Atomic size decreases going from ____ to ____.
left to right
-
1 mole of atoms is equal to _____ atoms?
- Avagadro's #
- 6.022x10²³ atoms
-
What is formula for % yield?
actual / theoretical X x% / 100
-
What determines if an atom is polar?
- If there is a e⁻ pr on the central atom
- Lewis structure is out of balance
-
What is the idea gas law?
PV=nRT
-
What is the formula for Boyle's Law?
P₁V₁ = P₂V₂
-
What is formula for Charle's Law?
V₁ / T₁ = V₂ / T₂
-
What is the formula for the combined gas law?
P₁V₁ / T₁ = P₂V₂ / T₂
-
What is 1 mole of any gas at STP equal to?
22.4L
-
At STP P=? T=?
- P= 760mmHg or 1 torr
- T= 0⁰ C or 273K
-
What causes pressure?
Atoms or molecules bouncing off the walls of the container
-
Describe Dalton's law.
All mater made up of tiny particles or atoms
-
Describe an ionic bond.
- Transfer of e⁻ to form ionic compound
- Usually metal & nonmetal
- Nonmetals gain e⁻
-
If an atom has 3 bonded atoms & 0 non bonding prs e⁻ the structure will be ____.
Trigonal Planer
-
If an atom has 2 bonded atoms & 0 non bonding prs e⁻ the structure will be ____.
Linear
-
If an atom has 2 bonded atoms & 1 non bonding prs e⁻ the structure will be ____.
Angular
-
If an atom has 4 bonded atoms & 0 non bonding prs e⁻ the structure will be ____.
Tetraherdal
-
If an atom has 3 bonded atoms & 1 non bonding prs e⁻ the structure will be ____.
Trigonal Pyramidal
-
If an atom has 2 bonded atoms & 2 non bonding prs e⁻ the structure will be ____.
Angular
-
What is the mass of 1 mole of oxygen?
16.0g
-
How many moles of carbon is 24.0 g?
2.00 moles
-
How may moles of water are 1.204x10²³ molecules of H₂O?
0.200 moles
-
After balancing N₂ + H₂ ---> NH₃ what # will be ifo H₂?
3
-
At what temp is the kinetic energy of molecules be "0"?
0 K
-
What happens to the vol of 1 mol of an ideal gas when the pressure is raised fr 4.00 atm to 8.00 atm @ constant temp?
Vol decreases to 1/2 original vol
-
What happens to the vol of 1 mole of an idea gas when temp is raised fr 40⁰ C to 80⁰ C @ constant pressure?
Vol increases by sm amt
-
What will vol of 28.0g of N₂ gas be @ STP?
22.4 L
-
What is formula for nitrogen dioxide?
NO₂
-
Describe a solution.
Homogeneous mixture
-
Describe a colloidal suspension.
- Heterogeneous mixture
- lg particles
-
Describe a suspension.
Particles so lg they settle out
-
What is the universal solvent?
Water
-
Electrolytes are formed from what?
Solutes soluable in ionic compounds
-
Describe non-electrolytes.
Formed fr non disociating molecular solutes
-
When a solid is placed in a liquid, as temp increased solubility does what?
Increases
-
What a gas is in H₂O as temp decreases solubility ____.
increases
-
Pressure has what effect on a solid in a liquid?
Very Little
-
Pressure has what effect on a gas in a liquid?
increase P = increase Solubility
-
What is osmosis?
Mvmt of solvent fr dilute solution to more concentrated solution thru semi-permiable membrane
-
What is osmotic pressure?
Pressure needed to stop osmosis
-
What is the formula for osmotic pressure?
- osmotic P = MRT
- M= molarity
- R= constant
- T= temp in K
-
What is the formula for concentration?
Amt of solute / Amt of solvent
-
Molarity = ?
Mol of solute / L of solution
-
What are 5 ways to increase reaction rate?
- Inc temp
- Inc surface area
- Add catalyst
- Inc concen of reactants
- Change nature of reactants
-
Describe a hypotonic solution.
- Lower concentration outside cell than inside
- Water moves in causing hemolysis
-
Hemolysis is caused by what?
- Water moving into a cell causing it to expand beyond its capacity
- Hypotonic solution
-
Describe a a hypertonic solution.
- Higher concentration outside cell than inside
- Water moves out causing crenation
-
What is crenation?
Cells shrivelling up caused by water moving out in a hypertonic solution
-
What is an isotonic solution?
One where concentrations inside & outside the cells are equal
-
What is the formula for the equilibrium constant?
Keq = [C] x [D] (products) over [A] x [B] (reactants)
-
When the Keq < 1 _____ are favored.
reactants
-
When the Keq >1 ____ are favored.
products
-
LeChatelier's Principle states . . . .
If a stress is placed on a sys in equilibrium the reaction will shift in a direction that lessens the stress
-
Name 3 strong acids.
- Hydrochloric - HCl
- Sulfuric - H₂SO₄
- Nitric - HNO₃
-
-
What are are 3 weak acids?
- HC₂H₃O₂ - Acetic acid
- NH₄¹⁺
- H₂CO₃ - Carbonic Acid
-
-
According to Bronsted Lowry an acid is an ______ & a base is an ______.
- H⁺ / proton donor
- H⁺ / proton acceptor
-
H₃O⁺ is aka ____ ion.
Hydronium
-
What is a conjugate acid/base pair?
A weak acid & the base that is left after the acid loses its H⁺
-
Define pH.
Degree of acidity or basicity of a solution
-
What is the equation pH is equal too?
-log [H₃O⁺]
-
What is the equation for the pOH?
-log [OH⁻]
-
How do we get H⁺ fr pH?
anti log of the neg of pH
-
[H₃O⁺] [OH⁻] = ?
1.0x10⁻¹⁴
-
What is the normal pH of blood?
7.35 - 7.45
-
What is the equation for a neutralization reaction?
V(acid) x M(acid) = V(base) x M(base)
-
Explain buffer solution.
Solutions containing components that enable the solution to somehow resist lg changes in pH when either an acid or base is added
-
What is the easiest way to achieve a buffer solution?
Add equal parts of a weak acid & its conjugate base
-
When a substance is oxidized it ____ ____.
- Loses e⁻
- LEO - Losing Electrons Oxidation
-
When a substance is reduced it ____ ____.
- Gains e⁻
- GER - Gaining Electrons Reduction
-
The reducing agent is . . . .
That which causes something to be reduced
-
The oxidizing agent is . . . .
That which is reduced
-
Define nuclear radiation (radioactivity).
Process by which atoms emit energetic particles or rays fr the nucleus
-
What is the charge & mass of an alpha particle?
-
What is speed & symbol of an alpha particle?
- 5-10% speed of light
- ⁴₂He²⁺
-
What is the charge & mass of an beta particle?
-
What is the charge & mass of an gamma particle?
-
What is speed & symbol of an beta particle?
- up to 90% speed of light
- ⁰₋₁e
-
What is speed & symbol of an gamma particle?
- Speed of light
- Bird like ϒ
-
What is a positron?
- Positive electron (antimatter)
- ⁰₁e
-
Half-life is defined as . . . .
Time required for 1/2 of a given quantity of a substance to undergo change
-
Different isotopes of the same element always have the same # of ____ but different #s of ____.
Protons, Neutrons
-
The # of protons & neutrons in ¹⁷₈O is . . . .
8p, 9n
-
When ²³⁴Th loses a beta particle, the resulting nuclear particle is ____.
²³⁴Pa
-
If ΔH is negative a reaction is (exothermic, endothermic)?
Exothermic
-
If ΔH is positive a reaction is (exothermic, endothermic)?
Endothermic
-
In acid, Litmus Paper turns what color?
Pink
-
In base, Litmus Paper turns what color?
Blue
-
What are colligative properties of a solution?
Properties that are concentration dependent
-
Steam fr a kettle hitting your hand & condensing is an (exo, endo) reaction?
Exothermic
-
The demonstration where we mixed 2 white powders in a flask & it stuck to the wooden block was an (exo, endo) reaction?
endothermic
-
When a reaction has more potential energy at the beginning than the end is an _____ reaction.
exothermic
-
What does adding a catalyst change on a reaction graph?
Activated complex
-
As concentration increases freezing point ____.
decreases
-
As concentration increases boiling point _____.
increases
-
As concentration increases osmotic pressure _____.
Increases
-
Molarity is equal to ______.
moles of solute / L of solution
-
Osmotic pressure is equal to ____.
π = MRT
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