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Chemistry Final > Semester 2 Review > Flashcards

Semester 2 Review Flashcards

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1
Q

What does temperature measure?

A

The average kinetic energy of particles in a sample of matter

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2
Q

Explain what is meant by the terms exothermic and endothermic

A

Exothermic is when a substance gives off heat, endothermic is when a substance absorbs heat.

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3
Q

What is meant by the specific heat capacity of a material?

A

Specific heat is the amount of heat required to raise the temp of one gram of that substance to 1 degree C

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4
Q

Calculate the mass (in grams) of each of the following substances that could be warmed over the indicated
temperature range by application of exactly 1.0 kJ of energy. (1.0 kJ = 1000J)
a. water, from 15°C to 42°C s=4.184 J/g °C
b. iron, from 25°C to 125°C s=0.45 J/g °C
c. carbon, from -10°C to 47°C s=0.71 J/g °C

A

a. 1000J/(4.18427°C)=8.85gH2O b. 1000J/(.45100°C)=22.2gFe
c. 1000J/(.71*57°C)=24.7gC

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5
Q

How many s,p,d and f orbitals can occupy any given energy level?

A

S-1, P-3, D-5, F-7

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6
Q

How many electrons can occupy an orbital at any given energy level?

A

2 electrons per orbital

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7
Q

What is the shape of a p-orbital? S-orbital?

A

P orbital- dumbbell shaped

S orbital- sphere shaped

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8
Q

What is the lowest energy level that can have a p-orbital? D-orbital? F-orbital?

A

P-orbital level 2
D-orbital level 3
F-orbital level 4

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9
Q

Is it possible for two electrons in the same atom to have exactly the same set of quantum numbers?

A

No, no two electrons can have the same quantum numbers

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10
Q

When is an electron configuration considered stable

A

When the subshells are full

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11
Q

Distinguish between an atom in its ground state and an excited atom

A

An atom in ground state had the lowest possible energy and an atom in excited state has gained energy

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12
Q

What happens when a photon of light is emitted?

A

A photon of light emits when an electron goes from excited states back to ground state

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13
Q

For the following elements list the electron configuration.
a. oxygen, cesium, krypton, titanium, scandium, nitrogen, chlorine

A

a. oxygen [He]2s2 2p4
1 cesium [Xe]6s
2 10 6 krypton [Ar]4s 3d 4p
22 titanium [Ar]4s 3d
21 scandium [Ar]4s 3d
23 nitrogen [He]2s 2p
25 chlorine [Ne]3s 3p

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14
Q

Define electronegativity

A

Electronegativity is the ability of an atom to attract electrons

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15
Q

Does electronegativity increase or decrease as the atomic number of an element increases within the same
period of the periodic table?

A

Electronegativity increases as atomic number increases. It increases from left to right across the periodic
table.

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16
Q

How is the strength of a bond between two elements in a molecule related to their electronegativities?

A

If the difference in electronegativities of two different atoms is very big, they will have a strong bond. If
the difference in electronegativities is very small, they will have a weaker bond.

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17
Q

What is the difference between an ionic and a covalent bond?

A

An ionic bond is between a metal and a non-metal. Great electronegativity difference.
A covalent bond is
between two non-metals. Very small electronegativity difference

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18
Q

Referring to the table of electronegativities, classify each of the following bonds as either ionic (I) or
covalent (C):
a.Al-Of

b. Al-S
c. Bi-Cl
d. Bi-O
e. C-Cl
f. N-O
g. Na-S
h. P-O
i. S-O
j. Ti-Br
k. Ca-F
l. Ba-S

A 
Ia.Al-O 
Cb.Al-S 
Cc.Bi-Cl 
Cd.Bi-O 
Ce.C-Cl 
Cf.N-O 
Ig.Na-S 
Ch.P-O 
Ci.S-O 
I j.Ti-Br 
Ik.Ca-F 
Il.Ba-S
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19
Q

What atoms forms diatomic molecules

A

Br2 I2 N2 Cl2 H2 O2 F2

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20
Q

Give an example of a polar covalent and a non polar covalent molecule

A

Polar covalent-two different atoms C-H

Non-polar- same atom N=N

21
Q

What does VSEPR stand for?

A

Valance Shell Electron Pair Repulsion

22
Q

What does the VSEPR theory predict?

A

It predicts the shape of molecules

23
Q

Draw the Lewis dot structure for SiO2

A

O=Si=O

24
Q

Convert 1.20 atm to units of mmHg, torr and pascals

A

1.20 atm * 760mmHg/1atm = 912 mmHg 1.20 atm * 760 torr/1atm = 912 torr
1.20 atm * 101,325 Pa/ 1atm= 121590 Pa

25
Q

What does STP stand for? What conditions correspond to STP?

A

Standard Pressure Temperature

STP= 0*C and 1 atm

26
Q

As temperature increases at constant pressure, what happens to volume?

A

Volume increases

27
Q

How is the concept of energy defined?

A

The ability to do work

28
Q

As a temperature increases at constant pressure, what happens to the volume?

A

The volume increases

29
Q

As volume increases at a constant temperature , what happens to the volume?

A

Volume decreases

30
Q

Define molar heat of fusion and molar heat of vaporization

A

Molar heat of fusion is the energy required to melt 1 mol of a substance
Molar heat of vaporization is energy required to change 1 mol of liquid to its vapor

31
Q

What is dipole-dipole attraction? What is hydrogen bonding?

A

Molecules whose positive and negative ends attract.

Hydrogen bonding is when nitrogen, fluorine, and oxygen interact

32
Q

Define London dispersion forces

A

Forces they exist between noble gases an non polar molecules

33
Q

What is vaporization?

What is condensation?

A

Vaporization is where liquid forms to make a gas

Condensation is where vapor molecules form a liquid

34
Q

Energy _as a substance goes from liquid to gas

A

Increases

35
Q

Energy _ as a substance goes from liquid to solid

A

Decrease

36
Q

How are kinetic energy and temperature related?

A

Temperature is a measure of the average kinetic energy

37
Q

Define homogenous and heterogenous mixtures

A

Heterogenous-mixture of two or more substances in same state.(oil and water)
Heterogenous mixture -mixture of two or more substances in different states (sand and water)

38
Q

What is a saturated, unsaturated and supersaturated solution?

A

Saturated- when a solution contains as much solute as will dissolve
Unsaturated- solution has not reached lint of solute
Supersaturated-contains more dissolved solid than a saturated solution can hold

39
Q

What is molarity?

A

Concentration of solute in solvent measured in mol/L

40
Q

What are the properties of and acids and bases

A

Acids- sour and turn litmus paper red

Bases-bitter, slippery, and turn litmus paper blue

41
Q

What is the pH of an acidic solution?

A

1-6

42
Q

What is the pH range of a base?

A

8-14

43
Q

When an acid and a base are mixed what are the results?

A

Water and salt

44
Q

What are the Arrhenius and Bronsted-Lowry definitions of acids and bases?

A

Arrhenius said acids produce H+ while bases produce OH-

Bronsted-Lowry said an acid is a proton donor while base is proton receptor

45
Q

What is a buffered solution?

A

A solution that resists change in pH. (ex) a weak acid and a conjugate base

46
Q

What do we mean by an equilibrium position?

A

It’s where the equilibrium lies, if there are more products than reactants (equilibrium lies to the right)
More reactants than products ( lies to the left)

47
Q

What is a catalyst?

A

A Catalyst lowers activation energy in a reaction

48
Q

What are four factors that affect reaction rate

A

Surface area, temperature, stirring and nature of reactants

49
Q

What is Le Chatelier’s principle?

A

When a change is imposed on a system at equilibrium, the position of the equilibrium shifts In a direction that tends to reduce the effects of change.

Chemistry Final (1 decks)

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