PS 100 Exam 3 study guide BYU

Triple bonds?

0

Double bonds?

1

1. Which type of bonding involves the sharing of electrons? a) Ionic bonding b) Covalent bonding c) Chemical bonding d) Physical bonding

B COVALENT BONDING

3. Which of the following is an unsaturated fat? a) Palmitic acid b) Oleic acid c) Laurie acid d) Stearic acid

B OLEIC ACID

Which of the following equations is balanced? A. NO22 + H22O --> HNO33 B. NaOH + HCl --> H22O + NaCl C. 2Ca + O22 --> 2MgO D. N22 + O22 --> 4NO

B. NaOH + HCl --> H22O + NaCl

What would be the charge of bromine, Br, in order to satisfy the octet rule? Hint: look at the column number. A. -2 B. -1 C. 1 D. 2

B. -1

What happens to the spacing between the energy of one Molecular Orbital (MO) and the next one immediately above or below it as the number of atoms that come together increases? A. Increases B. decreases C. remains the same

B. Decreases

Which type of atom has the highest ionization energy? A. metal B. non-metal

B. Non-Metal

How many electrons does Cl want to gain? Hint: how many are gained to form a stable noble gas electron configuration, ns2 np6 (octet rule)? A. Zero B. One C. Two D. Three

B. One

The source of differences between semiconductors and metal is caused by

Band Gaps

Characterize the following reaction as occurring with a favorable energy change for the system, a favorable entropy change for the atoms in the system, or both. Remember, gases have more disorder than liquids which have more disorder than solids. C33H88(gas) + 5O22(gas) → 3CO22(gas) + 4H22O(vapor), energy given off

Both

Characterize the following reaction as occurring with a favorable energy change for the system, a favorable entropy change for the atoms in the system, or both. Remember, gases have more disorder than liquids which have more disorder than solids. C66H1212O66(solid) + 3O22(gas) → 3CO22(gas) + 6H22O(vapor), energy given off

Both

2. Which of the following is not a mineral? a) Quartz b) Mica c) Arachidic acid d) Asbestos

C ARACHIDIC ACID

2. Which of these substances consists of individual molecules ? a) Diamond (C) b) Graphite (C) c) Water (H20) d) Sodium chloride (NaCl)e) Hydrogen (H2) f) Chlorine (CI,) g) Ammonia (NH3)

C, E, F, G

What happens to the overall entropy in the universe as this compound is formed? A. The entropy decreases. B. The entropy remains the same. C. The entropy increases.

C. The entropy increases

Predict how many electrons Mg would be expected to lose in ionic compounds. Hint: how many are lost to form a stable noble gas electron configuration, ns2 np6 (octet rule)? A. Zero B. One C. Two D. Three

C. Two

3. Which of the following pairs of elements would you expect to be covalently bonded (no ionic or metallic bond) ? a) 27 Co and 28 Ni b) 19 K and 9 F c) 15 P and 8 0 d) 11 Na and 53 I

C15 P and 8 O

What is the chemical formula for acetaldehyde?

C2H4O

Figure 1 shows that gas molecules are present inside a box. Figure 2 shows that there is a vacuum (no gas molecules present) inside of a box. If the two figures represent snapshots in time of an irreversible process, which figure came first and why?

Figure 2 came first because an empty box is more ordered.

The__________________ electrons act like a ________________ between the layers of nuclei when flattening metal with a mallet

Fluid-like, lubricant

Pure aluminum metal has a melting temperature at 660 °C. The process of liquid aluminum freezing to solid aluminum at this temperature is ___

IRREVERSIBLE

We see a large amount of order in the world around us from life to currents in the air and ocean. How is this consistent with the Law of Increasing Disorder?

It is because the sun provides additional high-order energy to the world to create this order.

Matching 1. ___ . The minimum amount of mass necessary for one fission to trigger another. 2. ___ A nucleus changes one of its protons into a neutron, or one of its neutrons into a proton. 3.____ A uranium atom splits into thorium and helium. 4. ___ A nucleon jumps from a high energy level to a lower one and emits a photon 5. ___ Two hydrogen atoms combine to make a helium atom. 6. ___ A uranium atom splits into xenon and strontium, plus a few neutrons. 7. ___ The amount of time required for 1/2 of the remaining radioactive nuclei to decay. 8. ___ A process where one event always triggers one or more additional events.

a. Alpha decay b. Fission c. Chain reaction d. Critical mass e. Beta decay f. Fusion g. Gamma decay h. Half-life

2. A difference between metals and semiconductors is caused by the different ____________________ and ___________________ of ______________________ electrons present in the two different types of materials.

sizes, energies, valence

1. The____________________ model helps answer questions about metals and semiconductors.

wave

6. ___ Semi-metals are electrically conductive and have high melting points.

T

7. ___ Semiconductors and metals are very similar in the way each forms alloys.

T

2. Generally, Molecular Oribitals (MOs) are low in energy because their electrons will be found between two nuclei.

T - When Electrons are found between two nuclei they are low in energy and binding molecules

2. ___ An unsaturated fatty acid with the same number of carbon atoms as a saturated fatty acid will generally melt at a lower temperature than saturated fatty acids

TRUE

3. ___ Molecular substances exhibit both covalent and intermolecular interactions.

TRUE

4. .___ The-COOH group is what makes an organic acid an acid.

TRUE

6. .___ Dispersion forces occur between non-polar molecules.

TRUE

6.____ The underlying atomic structure of both fatty acids and minerals determines many properties, such as melting point and crystal morphology.

TRUE

7. ___ Most forms of asbestos form fibers.

TRUE

True or False 1. ____ The melting point of saturated fatty acids increases with increasing number of carbon atoms.

TRUE

True/False 1. ___ Covalent bonding occurs between non-metal atoms.

TRUE

Fill in the Blank 1. ____________________combine with non-metals to form highly-colored compounds.

Transition metals

Metals Non Metals Large Atoms Small Atoms Few valence electrons Many valence electrons Low ionization energies High ionization energies

True

True/ False 1. ___ In the nucleus the strong force between two protons is stronger than the electric repulsion between two protons.

True/ False 1. (T) In the nucleus the strong force between two protons is stronger than the electric repulsion between two protons.

True/False 1. ___ Salts can easily be flattened or reshaped. 2.___ Ionic compounds have extremely low melting temperatures. 3.___ Molten salts are ionic conductors. 4.___ Metals easily lose electrons. 5.____ A salt is electrically neutral as a solid. 6.___Electrons like to go to the highest energy condition available to them.

True/False 1.(F) Salts can easily be flattened or reshaped. NO THEY ARE BRITTLE 2.(F) Ionic compounds have extremely low melting temperatures. NO THEY HAVE HIGH MELTING TEMPERATURES 3. (T) Molten salts are ionic conductors. 4.(T) Metals easily lose electrons. 5.(T) A salt is electrically neutral as a solid. 6.(F) Electrons like to go to the highest energy condition available to them. NO TO THE LOWEST ENERGY CONDITION AVAILABLE TO THEM

Which type of atom has valence electron states high enough in energy that they overlap with the stacked together molecular oribitals that form the conduction band? A. metal B. non-metal

A. metal

What would be the name of this ionic compound? A. Calcium Bromide B. Bromine Calcium C. Calcium Bromine D. Bromide Calcium

A. Calcium Bromide

Which of the following pair of atoms is most likely to form an alloy? a) 8 0 and 31 Ga b) 50 Sn and 82 Pb c) 7 N and l7 Cl

b) 50 Sn and 82 Pb

Which of the following is NOT why alloys are useful to us today? Alloys a) have lower melting temperatures. b) have a higher conductivity rate. c) are less malleable. d) reduce weight in objects.

b) NOT A REASON ALLOY IS USEFUL Alloys are not more conductive than pure metals a) REASON ALLOY IS USEFUL - Alloys have lower melting points, like tin alloys used for welding c) REASON ALLOY IS USEFUL- Alloys are less malleable like in steel, making it stronger - Iron, plus carbon has much greater tensile strength than iron or carbon separately d) REASON ALLOY IS USEFUL - Aluminum and magnesium alloys are much lighter, making them ideal for airplane construction

4. Determine the metal or non-metal nature of C and O. The compounds C02 and CO exist. What prediction can you make about their properties ? a) Metallic alloy, conducting b) Transparent gas c) Metallic alloy, nonconducting d) Britde, transparent solid, non-conducting

b) TRANSPARENT GAS

If GaAs forms a semiconductor like Ge, which of the following elements will form a semiconductor like Si? A. C and Ge B. B and As C. Ga and N D. Al and P

"Al and P".

1. Metal-metal compound. 2. Electrons act like a lubricant between layers of nuclei. 3. "Movement of electrons." 4. An electron that is not focused around any one nucleus. 5. Property of absorbing photons throughout the electromagnetic spectrum. 6. Substances that conduct electricity better than insulators but not as good as conductors. 7. The degree to which a substance conducts heat. 8. A measure of resistance to current flowing through a semiconductor. 9. Nuclei surrounded by a "sea" of electrons. 10. How easily light bounces off the surface of a substance.

1. Metal-metal compound. ALLOY 2. Electrons act like a lubricant between layers of nuclei. MALLEABILITY 3. "Movement of electrons." CONDUCTION 4. An electron that is not focused around any one nucleus. DELOCALIZED ELECTRONS 5. Property of absorbing photons throughout the electromagnetic spectrum. OPACITY 6. Substances that conduct electricity better than insulators but not as good as conductors. SEMICONDUCTORS 7. The degree to which a substance conducts heat. THERMAL CONDUCTIVITY 8. A measure of resistance to current flowing through a semiconductor. RESISTIVITY 9. Nuclei surrounded by a "sea" of electrons. METALLIC BONDING 10. How easily light bounces off the surface of a substance. REFLECTIVITY

Each molecule of methane has the formula 𝐶𝐻4CH4. If there are 4000 carbon atoms present how many hydrogen atoms will be required to convert all of the carbon atoms into methane?

16000

2. The electromagnetic force extends over a longer distance than the strong nuclear force.

2. (T) The electromagnetic force extends over a longer distance than the strong nuclear force.

CH4 + 2O2 --> ?H20 + CO2

2H2O + C02

?Mg + O2 --> ?MgO2

2Mg + 02 --> 2MgO

3. ___ Charge is always conserved in any nuclear process.

3. (T) Charge is always conserved in any nuclear process.

3. For a given period, metals have _______________ atomic volumes, whereas non-metals have________________ atomic volumes.

3. For a given period, metals have LARGE atomic volumes, whereas non-metals have SMALL atomic volumes.

How many bonds does each carbon have in propanal?

4 C3H8

4.____ Mass changes in nuclear processes.

4. (T) Mass changes in nuclear processes.

In acetaldehyde, how many single bonds are there?

5

5. ___ If two large nuclei were to combine, the process would release energy.

5. (F) If two large nuclei were to combine, the process would release energy

When you look at a mass spectrum for butanal (or butyraldehyde), the next member of the aldehyde family after propanal, what is the largest mass that will have a peak on the graph? (Hint: you must determine its chemical formula.)

72 Atomic Mass of oxygen 16 Atomic Mass of carbon 12 x 4 = 48 Atomic Mass of Hydrogen 1 x 8 = 8 16 + 48 + 8 = 72

What happens to the number of Molecular Orbital's as the number of atoms that come together increases? A. Increases B. Decreases C. Remains the same

A. Increases

Which type of atom has valence electrons higher in the energy well? A. metal B. non-metal

A. Metal

What happens to the energy of the Mg and Cl atoms as this compound is formed? A. The energy decreases. B. The energy remains the same. C. The energy increases.

A. The energy decreases

5. The most energetically favorable arrangement of ions maximizes____________ forces and minimizes repulsive ones.

ATTRACTIVE

4. Fatty acid molecules consist of a hydrocarbon tail attached to a) -Si04 b) -MgFe c) -C02 d) -COOH

D -COOH

What would be the charge of calcium, Ca, in order to satisfy the octet rule? Hint: look at the column number. A. -2 B. -1 C. +1 D. +2

D. +2

How many nonmetals atoms (bromine) are needed to take all of the electrons that the metal atoms (calcium) want to give? A. 1 Bromine atom, 1 Calcium atom B. 2 Bromine atoms, 2 Calcium atoms C. 1 Bromine atom, 2 Calcium atoms D. 2 Bromine atoms, 1 Calcium atom

D. 2 Bromine atoms, 1 calcium atom

When do polyatomic ions form crystals? A. When they combine with metal atoms to form salts. B. When they combine with other non-metal atoms. C. never. D. A and B.

D. A and B

What would be the chemical formula of the ionic compound between calcium and bromine? A. CaBr B. Ca2Br2 C. Ca2Br D. CaBr2

D. CaBr2

4. Metals lose______________ to form positive ions.

ELECTRONS

Characterize the following reaction as occurring with a favorable energy change for the system, a favorable entropy change for the atoms in the system, or both. Remember, gases have more disorder than liquids which have more disorder than solids. H22(gas) + O22(gas) → H22O(vapor), energy given off

Energy

Characterize the following reaction as occurring with a favorable energy change for the system, a favorable entropy change for the atoms in the system, or both. Remember, gases have more disorder than liquids which have more disorder than solids. NH44NO33(solid) + H22O(liquid) → NH44++ + NO33−− in solution, energy absorbed

Entropy

A car can't convert all of the energy from its fuel to macroscopic kinetic energy. Why?

Entropy (or disorder) would decrease. Entropy must always increase.

4. . For an alloy to form, the atoms must be different sizes.

F - Alloys can be made up of metals with atoms of the same size or different sizes.

True/False 1: ___ Light can only be seen through very thin metal.

F - LIGHT CAN'T BE SEEN THROUGH THIN METAL - IT IS OPAQUE - OPACITY

3. Compositions of alloys are generally fixed in simple ratios.

F - They are not fixed in any ratio Gold and platinum can be 50% Gold, 50% Platinum or 98% Gold, 2% Platinum

5. ___ Often alloys are better conductors than either of the metals, in their pure form, that make up the alloy.

F- Alloys are always worse conductors than the metals in pure form.

2. ___ Metal and non-metal substances combine to form molecules.

FALSE

3. ___ Ionic bonds hold fatty acid molecules together in the solid state.

FALSE

4. ___ Covalent molecules do not have well-defined shapes.

FALSE

5. ___ The silicate ion (Si04)4- is flat (planar) with the following structure: O O—Si—O O

FALSE

5. ___ The triple covalent bond of carbon monoxide (CO) is a type of weak chemical interaction.

FALSE

8 ___ Crystals of quartz flake off in thin sheets

FALSE

(T/F) Current can flow in all directions in an LED. A. True B. False

False

Matching 1. ____ A characteristic of ionic substances, such as salts, that readily shatter when struck a sharp blow. 2. ___ A characteristic of salts that readily transmit light; opposite of opaqueness. 3. ___ The chemical bond that binds metallic ions to non-metallic ions by electrical attraction. 4. .___ A charged particle formed when an atom or molecule loses or gains electrons. 5. .___ A substance formed from the ionic bond of a metal with a non-metal. 6. ___ A chemical compound that ionizes when dissolved or molten to produce an electrically conductive medium.

Matching 1. (C) BRITTLENESS A characteristic of ionic substances, such as salts, that readily shatter when struck a sharp blow. 2. (F) TRANSPARENCY A characteristic of salts that readily transmit light; opposite of opaqueness. 3. (B) IONIC BONDING The chemical bond that binds metallic ions to non-metallic ions by electrical attraction. 4. (E) ION A charged particle formed when an atom or molecule loses or gains electrons. 5. (A) SALT A substance formed from the ionic bond of a metal with a non-metal. 6. (D) ELECTROLYTE A chemical compound that ionizes when dissolved or molten to produce an electrically conductive medium.

Matching 1. ___The chemical bond between two non-metals characterized by sharing of valence electrons. 2. ___ A separation of charge with one positive side and one negative side 3. ___ A material in which another material dissolves. 4. ___ Having a pH value less than 7, meaning that the hydronium ion concentration is greater than in pure water. 5. ___ Chemical compounds between the elements carbon and hydrogen. The compounds that make up gasoline are examples. 6. ___ Ions composed of more than one covalently-bound atom. 7. ___ A covalent bond involving two pairs of electrons shared between the two bound atoms. 8. ___ Bonds or molecules having an unequal polar molecules. 9. ___ Forces between molecules.

Matching 1. (E) COVALENT BOND The chemical bond between two non-metals characterized by sharing of valence electrons. 2. (G) DIPOLE A separation of charge with one positive side and one negative side 3. (H) SOLVENT A material in which another material dissolves. 4. (I) ACIDIC Having a pH value less than 7, meaning that the hydronium ion concentration is greater than in pure water. 5. (F) HYDROCARBONS Chemical compounds between the elements carbon and hydrogen. The compounds that make up gasoline are examples. 6. (A) MOLECULAR IONS Ions composed of more than one covalently-bound atom. 7. (C) DOUBLE BOND A covalent bond involving two pairs of electrons shared between the two bound atoms. 8. (D) POLAR Bonds or molecules having an unequal polar molecules. 9. (B) INTERMOLECULAR FORCE Forces between molecules.

Matching 1. ___ . The minimum amount of mass necessary for one fission to trigger another. 2. ___ A nucleus changes one of its protons into a neutron, or one of its neutrons into a proton. 3.____ A uranium atom splits into thorium and helium. 4. ___ A nucleon jumps from a high energy level to a lower one and emits a photon 5. ___ Two hydrogen atoms combine to make a helium atom. 6. ___ A uranium atom splits into xenon and strontium, plus a few neutrons. 7. ___ The amount of time required for 1/2 of the remaining radioactive nuclei to decay. 8. ___ A process where one event always triggers one or more additional events.

Matching 1. (d) CRITICAL MASS The minimum amount of mass necessary for one fission to trigger another. 2. (e) BETA DECAY A nucleus changes one of its protons into a neutron, or one of its neutrons into a proton. 3. (a) ALPHA DECAY A uranium atom splits into thorium and helium. 4. (g) GAMMA DECAY A nucleon jumps from a high energy level to a lower one and emits a photon 5. (f) FUSION Two hydrogen atoms combine to make a helium atom. 6. (b) FISSION A uranium atom splits into xenon and strontium, plus a few neutrons. 7. (h) HALF LIFE The amount of time required for 1/2 of the remaining radioactive nuclei to decay. 8. (c) CHAIN REACTION A process where one event always triggers one or more additional events.

Matching 1.___Contains C=C double bonds. 2.___ Contains only C-C single bonds. 3.___ Best geometric arrangement of four single bonds around a central atom. 4.___ Building block of many minerals. 5.___ Organization of matter in which atoms or ions are arranged in an orderly, repeating patterns. 6.___ Silicate mineral in which all silicate tetrahedra are bonded with equal strength to four other tetrahedra. 7. ___ Silicate mineral that has a super "foot-long" structure. 8. ___ Silicate mineral that has a layer-like structure.

Matching 1. (h) UNSATURATED FATTY ACIDS Contains C=C double bonds. 2. (b) SATURATED FATTY ACIDS Contains only C-C single bonds. 3. (f) TETRAHEDRON Best geometric arrangement of four single bonds around a central atom. 4. (a) SILICATE ION (Si044~) Building block of many minerals. 5. (g) CRYSTAL Organization of matter in which atoms or ions are arranged in an orderly, repeating patterns. 6. (d) QUARTZ Silicate mineral in which all silicate tetrahedra are bonded with equal strength to four other tetrahedra. 7. (c) ASBESTOS Silicate mineral that has a super "foot-long" structure. 8. (e) MICA Silicate mineral that has a layer-like structure.

7. When writing down the chemical formula for a salt, the____________ symbol is written first and the ________________ is written second

Metal, non-metal

Magnesium chloride forms a solid in which two chloride ions are found for every magnesium ion but no discrete molecules are observed in the solid. What is the simplest formula for this compound?

MgCl2

What classification of matter is magnesium chloride?

Network matter In network matter there are no individual molecules, and the entire crystal or amorphous solid may be considered a macromolecule. (one big molecule)

Can sulfur be considered a compound and why?

No, it is composed of only one type of atom

6. Each ion of an ionic compound has the ions of the_________ charge as its next-door neighbors.

OPPOSITE

What is the chemical formula for sulfur?

S8

Matching 1. ___The chemical bond between two non-metals characterized by sharing of valence electrons. 2. ___ A separation of charge with one positive side and one negative side 3. ___ A material in which another material dissolves. 4. ___ Having a pH value less than 7, meaning that the hydronium ion concentration is greater than in pure water. 5. ___ Chemical compounds between the elements carbon and hydrogen. The compounds that make up gasoline are examples. 6. ___ Ions composed of more than one covalently-bound atom. 7. ___ A covalent bond involving two pairs of electrons shared between the two bound atoms. 8. ___ Bonds or molecules having an unequal polar molecules. 9. ___ Forces between molecules.

a. Molecular ions b. Intermolecular force c. Double bond d. Polar e. Covalent bond f. Hydrocarbons g. Dipole h. Solvent i. Acidic

Matching 1. ____ A characteristic of ionic substances, such as salts, that readily shatter when struck a sharp blow. 2. ___ A characteristic of salts that readily transmit light; opposite of opaqueness. 3. ___ The chemical bond that binds metallic ions to non-metallic ions by electrical attraction. 4. .___ A charged particle formed when an atom or molecule loses or gains electrons. 5. .___ A substance formed from the ionic bond of a metal with a non-metal. 6. ___ A chemical compound that ionizes when dissolved or molten to produce an electrically conductive medium.

a. Salt b. Ionic Bonding c. Brittleness d. Electrolytes e. Ion f. Transparency

Matching 1.___Contains C=C double bonds. 2.___ Contains only C-C single bonds. 3.___ Best geometric arrangement of four single bonds around a central atom. 4.___ Building block of many minerals. 5.___ Organization of matter in which atoms or ions are arranged in an orderly, repeating patterns. 6.___ Silicate mineral in which all silicate tetrahedra are bonded with equal strength to four other tetrahedra. 7. ___ Silicate mineral that has a super "foot-long" structure. 8. ___ Silicate mineral that has a layer-like structure.

a. Silicate ion (Si044~) b. Saturated fatty acids c. Asbestos d. Quartz e. Mica f. Tetrahedron g. Crystal h. Unsaturated fatty acids

The atomic orbitals for potassium (K) and bromine (Br) are similar to those for sodium and chlorine in Figure 22.2 in that the potassium atomic orbitals are higher in energy than their counterparts on bromine. Why is this? a) Potassium valence electrons are closer on average to their nucleus than bromine valence electrons. b) Potassium valence electrons experience a stronger attraction to their nucleus because of a larger atomic volume and smaller nuclear charge. c) Bromine valence electrons experience a stronger attraction to their nucleus because of smaller atomic volume and increased nuclear charge. d) Bromine valence electrons experience a weaker attraction for their nucleus because there are fewer positively charged protons.

c) Bromine valence electrons experience a stronger attraction to their nucleus because of smaller atomic volume and increased nuclear charge.

Which of the following is a characteristic of metallic bonds? a) brittle b) transparent c) shiny d) low melting temperature e) insulator

c) SHINY - METALS ARE REFLECTIVE! a) WRONG metals are MALLEABLE not brittle b) WRONG metals are OPAQUE not transparent d) WRONG metals have HIGH melting temperatures e) WRONG metals are CONDUCTORS not insulators

2. Electrons go to the____________ energy condition available to them.

lowest