Chapters 10, 11 & 12

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linear molecular geometry

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First chem test

59 Terms

1

linear molecular geometry

  • 180 degrees

  • ex: BeCl2, HgCl2, CO2

  • Orbital: sp

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2

Trigonal planar

  • 120 degrees

  • ex: BF3, CO3²-, NO3-, SO3

  • orbital: sp²

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3

Tetrahedral

  • 109.5 degrees

  • ex: CH4, PO4Âł-, TiCl4

  • orbital: spÂł

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4

sigma bond

A sigma bond is a strong covalent bond formed by overlapping atomic orbitals along the bonding axis, enabling electron sharing between atoms.

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5

pi bond

A pi bond is a covalent bond formed by overlapping atomic orbitals in a side-by-side manner. It occurs when two p orbitals align parallel to each other and share electrons. Pi bonds are found in double and triple bonds, adding stability and strength to the molecule.

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6

Element Be in electron configuration, Molecular orbital configuration, and bond order

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7

bond order formula:

½ (antibonding-bonding)

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8

Element N2 in electron configuration, Molecular orbital configuration, and bond order

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9

unpaired electrons:

attracted

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10

paired electrons:

unattracted

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11

Carbon disulfide, Cs2, has a normal boiling point of 46 degrees celsius and a heat of vaporization of 26.8kJ/mol. What is the vapor pressure of carbon disulfide at 35 degrees celsius in mmh Hg?

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12

Selenium tetrafluoride is a colorless liquid. It has a vapor pressure of 757 mmHg at 105 degrees celsius and 522 mmHg at 95 degrees celsius. What is the heat of vaporization of selenium tetrafluoride?

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13

London Dispersion Forces

  • weakest force

  • hydrocarbon

  • Higher LDF

  • Longer the molecular chain = Higher molecular weight

  • ex: Ch4

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14

Dipole - Dipole

  • H-Cl…H-Cl

  • CH3CH2CH3

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15

Hydrogen Bonding

  • super dipole

  • Only when H is connected to F, O, & N

  • ex: H2O

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16

What time of bond is propanol (CH3CH2CH2OH)?

  • hydrogen Bonding

  • LDF

  • Dipole-Dipole

  • It has all 3 but hydrogen bonding is the strongest

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17

What type of bonding is methane (CH4)?

  • LDF

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18

What type of bonding is fluoromethane (CH3F)

  • LDF

  • Dipole - Dipole

  • It has both but Dipole - Dipole is stronger

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19

Arrange the following hydrocarbons in order of increasing vapor pressure: ethane(C2H6), propane(C3H8), butane(C4H10), hexane (C6H14)

  • C6H14 < C4H10 < C3H8 <C2H6

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20

Molecular solid:

  • gas elements

  • ex: C02(s) = dry ice

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21

Metallic solid:

  • just metal elements

  • conductors

  • Ex: Cu —> 3s3p4s3d

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22

Ionic solid:

  • Nonmetal + metal

  • insulators

  • ex: NaCl, Zns, CsCl

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23

Covalent bonds

  • Strongest bond

  • can either lose or gain 4e’

  • ex: diamond, graphite, asbestos

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24

Classify the following Zinc, Zn according to the forces of attraction that exist between the structural units

  • Metallic solid

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25

Classify the following Sodium iodide, NaI according to the forces of attraction that exist between the structural units

  • Ionic solid

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26

Classify the following Silicon carbide, SiC according to the forces of attraction that exist between the structural units:

  • covalent solid

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27

Classify the following methane, Ch4 according to the forces of attraction that exist between the structural units:

  • molecular solid

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28

Arrange the following elements in order of increasing melting point: Silicon, hydrogen, lithium

  • H < Li < Si

  • The higher the IMF = higher MP

  • The higher the MW = higher IMF

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29

Describe what type of solid is formed for each of the following substances and arrange these in order of increasing melting point:

  • C2H5OH = Molecular solid, Hydrogen bonding

  • CH4 = Molecular solid, LDF

  • CH3Cl = Molecular solid, Dipole - Dipole

  • MgSO4 = Ionic Solid

  • CH4 < CH3Cl < C2H5OH < MgSO4

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30

Solute:

  • The smaller amount

  • the gas or solid dissolved into a liquid

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31

Solvent:

  • The greater amount

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32

Miscible fluids:

  • Fluids that mix with or dissolve in each other in all proportions

  • ex: Air

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33

Solubility:

  • The amount of substance that dissolves in a given quantity of water at a given temperature

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34

Which ion has the larger hydration energy, NA+ or K+?

  • Na+

  • The higher the radius the smaller the hydration energy, vice versa

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35

A liter of water at 25 degrees celsius dissolves 0.0404 g O2 when the partial pressure of the oxygen is 1.0 atm. What is the solubility of oxygen from air, in which the partial pressure of O2 is 159 mmHg

  • 8.44Ă—10^-3 g-L

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36

Mass % of solute:

  • the % by mass of the solute contained in a solution

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37

Mass % of solute:

  • mass of solute - the mass of solution x 100

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38

ppb =

  • 1 mg for every 109g of solution

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39

ppm =

  • 1g solute for every 10^6g solutions

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40

Calculate the mass percentage of NaCl in a solution containing 1.50g of NaCl in 50.0g of water.

  • 2.91%

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41

Molality =

  • moles of solute - kg of solvent

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42

G —> moles

  • use when solving for moles

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43

G —> kg

  • use when solving for solvent

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44

Toluene, C6H5CH3, is a liquid compound similar to benzene, C6H6. It is starting material for other substances, including trinitrotoluene. Find the molality of toluene in a solution that contains 35.6g of toluene nd 125 g of benzene

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45

What are the mole fractions of glucose and water in a solution containing 5.67g of glucose, C6H12O6, dissolved in 25.2g of water?

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46

A sample with the density of 0.876g/mL contains 5.0g of toluene (C7H8) and 225g of benzene. Calculate the molarity of the solution

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47

White phosphorus, P4, is a white waxy solid melting at 44C to a clear liquid. The liquid has a vapor pressure of 400.0 mmHg at 251C and 760 mmHg at 280C. What is the heat of vaporization of this substance?

  • 53.29 kj/mol

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48

mothballs slowly becoming smaller and eventually disappear

  • Sublimation

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49

Raindrops hit a cold metal surface, which becomes covered with ice

  • Freezing

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50

Rubbing alcohol spilled on the palm of your hand feels cool as the volume of liquid decreases

  • Evaporation

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51

List the following substances in order of increasing boiling point: CH3OH, C2H5OH, C2H6, CH4

  • CH4 < C2H6 < CH3OH < C2H5OH

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52

Which substance has the lower boiling point: LiCl or HCl

  • HCl

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53

Which substance has the lower boiling point: NH3 or PH3

  • PH3

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54

In each of the following pair of molecules, which compound experiences the strongest london dispersion force: CCl4 or CF4

  • CCl4 because it has a higher molecular weight

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55

Draw a molecular oribital energy diagram for the O2 ion. Write the molecular orbital configuration and determined the bond order for this ion

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56

How much heat is required to vaporize 546.0g of NH3? The heat of vaporization is 23.4 kJ/mol.

7.50×10²kJ

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57

Ethanol (C2H5OH) melts at -114C and boils at 78C. The enthalpy of fusion of ethanol is 5.02 kJ/mol and its enthalphy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 and 2.3 J/g*K, respectively. How much heat is required to convert 49.0 g of ethanol at 35C to the vapor phase at 78C

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58

Which hybridization schemes allows for the formation of at least one pi bond: sp³, sp², sp³d²

  • sp²

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59

Which hybridization scheme allows the central atom to form more than 4 bonds: spÂł, spÂłd, sp62

  • spÂłd

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