Final Chem 141

Question 1

2 polyatomic molecules?

Answer 1

Phosphorus⇒ P₄

Sulfur⇒ S₈

Question 2

Usually soluble compounds?

Answer 2

1. Group 1A
2. chlorides
3. chlorates
4. nitrates
5. ammonium

Question 3

Usually Insoluble compounds?

Answer 3

1. carbonates
2. phosphates
3. hydroxides
4. sulfides

Question 4

7 strong acids

Answer 4

1. Chloric Acid HClO₃
2. perchloric Acid HClO₄
3. Hydrochloric Acid HCl
4. Hydroiodic Acid HI
5. Hydrobromic Acid HBr
6. Sulfuric Acid H₂SO₄
7. Nitric Acid HNO₃

Question 5

Exothermic Reactions:

Change H(enthalpy)= _______

Change S(entropy)=______

Change G(free energy/spontaneousness)=______

Answer 5

enthalpy= (-) negative

entropy= (-) negative

free energy= non-spontaneous

Question 6

Endothermic Reactions:

change H(enthalpy)=_______

change S(entropy)=_______

change G(free energy/spontaneousness)=______

Answer 6

enthalpy= (+)positive

entropy= (+)positive

free energy= spontaneous

Question 7

Enthalpy (change H) is_______

Answer 7

the internal heat(energy) of a reaction

Question 8

Entropy (change S) is ___________

Answer 8

the disorder of a system(lack of predictability)

Question 9

energy levels increase with ______

Answer 9

of n (prinipal energy level)

lowest energy⇒top of periodic table

highest energy⇒ bottom of periodic table

Question 10

lowest energy levels have ______ wavelengths

Answer 10

shortest wavelengths

therfore highest frequency

Question 11

highest energy levels have ______ wavelengths

Answer 11

longest

therefore the lowest frequency

Question 12

if given a lab experiment problem with # of trials with values use_______

Answer 12

average of values not including any outliers

Question 13

Standard pressure is ________

Answer 13

1.00 Bar=0.987 atm

Question 14

Standard Temperature is ________

Answer 14

0 Celsius= 273.15 K

Question 15

metallic character on periodic table

increases _______

Answer 15

down to bottom left

Question 16

atomic size on periodic table increases______

Answer 16

down to bottom left

Question 17

ionization energy on periodic table increases___

Answer 17

up to right

Question 18

electronegativity on periodic table increases_____

Answer 18

up to right

Question 19

transition metal ions:

lose __ electrons before __ electrons

Answer 19

lose s electrons before d electrons

Question 20

endothermic reactions become: ___ spontaneous as termperature decreases because_____

Answer 20

more spontaneous as temperature decreases because now they have more free energy now in the system which makes it more unpredictable or “spontaneous”

Question 21

exothermic reactions: become ___ spontaneous as their temperature increases because now they have_______

Answer 21

become less spontaneous as their temperature increases because now they have less free energy in the system because the system is releasing energy so therefore the system is less unpredictable or is “non-spontaneous”

Question 22

Helium(He) has 2 electrons in the 1s orbital, when it becomes singly ionized, forming He⁺

⇒its spectrum resembles that of the _______

Answer 22

hydrogen spectrum

Question 23

ionization energy is ______

Answer 23

energy required to remove one electron from a gaseous atom of an element

Question 24

dueterium is a_____

Answer 24

isotope of hydrogen

Question 25

“chemically inert” refers to _______

Answer 25

noble gases

because they have an oxidation # of 0 due to having the maximum # of valence electrons in their shell(2 for helium, 8 for rest) making them stable and prevents them from forming compounds readily

Question 26

paramagnetic?

Answer 26

is elements with partial filled orbitals

(unpaired e^-)

Question 27

diamagnetic?

Answer 27

elements with filled orbitals

(only paired e^-)

Question 28

electropositive?

Answer 28

is the opposite of electronegative

electronegative⇒atoms ability to attract electrons

electropositive⇒atoms ability to repel electrons

Question 29

tetrahedral bond angle?

4 regions e^-

4 bonded pairs

Answer 29

109.5

Question 30

trigonal planar bond angles

Answer 30

120

Question 31

tetrahedral -triangular pyramid bond angle?

4 regions e^-

3 bonded pairs

Answer 31

≈107

Question 32

tetrahedral-angular bond angle?

4 regions e^-

2 regions bonded

Answer 32

≈104.5

Question 33

electron affinity ?

Answer 33

is ability to accept electrons to form negative ions

Question 34

resonance structures are?

Answer 34

an average of the principal lewis dot structures of the molecule

Question 35

what concept describes the formation of four equivalent, single, covalent bonds by carbon in its compounds that resemble methane, CH₄

Answer 35

hybridization

Question 36

group 4A elements as central atom can form what kind of covalent bonds?

think of silicon

like SiO₂

Answer 36

network solid covalent bonds, meaning they pretty much keep linking together

so silicon dioxide forms a tetrahedral form with 109.5 bond angles instead of the linear shape you would get from the lewis structure giving 180 bond angles