General Chemistry (1.1-3.1 videos)

What is the proton number of a Beta particle? Mass number?

-1, 0

What are the bond angles in XeF4?

90°

Which of the following is a network covalent solid? Rb2SO4 NH3 C(diamond) TiO2

C(diamond)

Which of the following has the largest atomic radius? B Al Ga In

In (Hint:As long as the ions being compared all have the same charge, then the trend for ionic radius will be the same as that for atomic radius. Atomic radius increases going down a group (column) and to the left across a period (row) on the periodic table. The answer choices are all in the same group and I- is the furthest down the group and therefore has the largest ionic radius.)

Solid---> Liquid is called

Melting/Fusion

Which of the following atoms have a filled octet? Ne Mg Na F

Ne (Hint: All atoms want to have a full octet, Neon with a configuration of 2s2 2p6 and is the only one with 8 electrons in the outer shell.)

Quantum Numbers- Number: n, Name: Principal, Range [1..infiniti] What is this?

Shell

Which of the following is a network covalent solid? SiO2 H2O2 NaCl LiOH

SiO2

Anions are _____ than the neutral species.

bigger

Gas----> Solid is called

deposition

Atoms with unequal numbers of protons and electrons produce charged atoms or _____.

ions

alpha decay is the only one that reduces _____ number.

mass

A proton and electron combined together makes a _____.

neutron

Shells are numbered as n=1,2,3,4, etc. and increase in _____ and _____ as they get further away from the _____.

size, energy

Cations are _____ than the neutral species.

smaller

What is the hybridization of the central atom in SO2? sp sp2 sp3 dsp3

sp2

What is the hybridization of the central atom in XeF2? sp sp2 sp3 sp3d

sp3d

What is the correct Lewis Structure for BF3?

(Hint: 1) First find the total number of valence electrons: 3 + 3(7) = 24 electrons. 2) Next set up the molecular skeleton with the atom that can make the most bonds (boron in this case) in the middle. 3) Fill up the octets of the outer F atoms. 4) There are no electrons left at this point. 5) The central atom does not have a filled octet but recall that boron is one of the exceptions that is allowed to go under the octet rule with only 6 electrons.)

What is the correct Lewis structure for H2CO?

(Hint: 1) First find the total number of valence electrons: 4 + 6 + 2(1) = 12 electrons. 2) Next set up the molecular skeleton with the atom that can make the most bonds (carbon in this case) in the middle. 3) Fill up the octets of the outer oxygen atom. The hydrogen atoms are already full. 4) There are no electrons remaining. 5) The central carbon atom isnt happy and still needs 2 more electrons so well have the oxygen donate a lone pair and make a double bond to the carbon atom.)

What is the effective nuclear charge felt by a 1s in Mg?

+12

Based off these properties below, name the specific group from the periodic table. 1.) Have a full octet 2.) Don't have a whole lot for chemical reactivity

Noble Gas

For which of the following phase changes is Delta H > 0 and S <0? Fusion Sublimation Deposition None of these

None of these

For Elements below atomic number 20 the N/Z ratio should be? The N/Z ratio should be greater than one The N/Z ratio should be equal to one The N/Z ratio should be less than one None of the above are correct

The N/Z ratio should be equal to one

Is this a possible set of quantum numbers in an atom? [3, 1, 0, +1/2]

Yes

Gas---> Liquid is called

condensation

When the nucleus sucks in one of the inner core electrons, this is called _____ _____.

electron capture

A(n) _____ nucleus is likelier to be more radioactive.

unstable

If you have an odd number of protons and neutrons there is a high chance that the nucleus is _____.

unstable

Ionization energy increases as you move _____ the group and to the _____ going towards He.

up, right

Which of the following is most likely to decay by alpha emission? uranium-235 carbon-14 helium-4 sodium -23

uranium-235

The effective nuclear charge is equivalent to the number of _____ _____.

valence electrons

Liquid---> Gas is called

vaporization

Alkaline earth metals are not as reactive with _____ as alkali metals.

water

which decay converts a neutron into a proton?

B decay

Name this principle: No 2 elections in an atom can have the same 4 quantum numbers

Pauli Exclusion Principle

What is the shorthand electron configuration for Zn 2+?

[Ar], 3d10

What is the shorthand electron configuration for K?

[Ar], 4s1

What is the shorthand electron configuration for Cu?

[Ar], 4s1, 3d10

If you have a magic number of protons and neutrons your nucleus is most likely to be very _____.

stable

If you have an even number of protons and neutrons your nucleus is _____.

stable

Solid---> Gas is called

sublimation

Shells can be subdivided into _____. The maximum number of subshells is equivalent to the shell number.

subshells, subshells

Formula for finding the effective nuclear charge.

z (protons in the nucleus) - s (sheilding

A gamma ray has an atomic number of _____ and resting mass of _____.

0, 0

How many valence electrons does Potassium have?

1

A neutron has a mass number of _____ and a proton number of _____.

1, 0

A proton has a mass number of _____, and a proton number of _____.

1, 1

In order to have a stable nucleus your n/z has to be greater than _____ for elements higher than atomic number _____.

1, 20

In order to have a stable nucleus, your n/z ratio has to be approximately = _____ for elements up to atomic number _____.

1, 20

The half-life of a radioactive nuclide is 2.5hrs. What fraction of a sample of this nuclide would remain after 12.5 hrs? 1/8 1/16 1/32 1/64

1/32

How many electrons maximum can occupy the third shell (n = 3) of an atom? 9 16 18 32

18

What is the percent sodium in Na2S2O8?

19%

When n=1, the only subshell possible is the _____ subshell. When n=2, two subshells are possible the _____ and _____. When n=3, three subshells are possible the 3s, 3p, and _____

1s, 2s, 2p, 3d

What is the electronic configuration of Cl-?

1s2, 2s2, 2p6, 3s2, 3p6

How many lone pairs of electrons are around the Xe atom in XeF4? 1 2 3

2

How many lone pairs of electrons are on the central atom of IBr3? 1 2 3 4

2

How many valence electrons does Zn have?

2

For every neutron Uranium absorbs it usually gives off between _____ -_____ neutrons.

2, 3

What is the percent oxygen in AgNO3?

28.1 % (Hint: The formula weight for AgNO3 is 109 + 14 + 3(16) = 171 There are three oxygen atoms that weight a total of 48.)

What is the percent composition of the Copper (Cu) in the following molecule? CuBr2

28.4

What percentage of a radioactive nuclide remains after the passing of 5 half-lives? 1.56% 3.13% 6.25% 87.5%

3.13%

What is the maximum number of electrons that could occupy the 4th shell of an atom? 4 8 18 32

32 (Hint:There are n2 orbitals in each shell and each orbital can hold a maximum of 2 electrons and so the maximum number of electrons held by any shell is 2n2. For the 4th shell there are 42 or 16 orbitals which can hold a maximum of 32 electrons.)

How much heat is required to raise 50g of H20 from 10 degrees C to 79.4 degrees C? (specific heat of water = 1cal/g degrees C) 6940cal 694cal 13880cal 3470cal

3470cal

An alpha particle has a mass number of ____ and a proton number of ____.

4, 2

What is the percent oxygen by mass in NaOH?

40.0 (Hint: NaOH has an atomic mass of about 40. Oxygen has an atomic mass of about 16. So %O = (16/40)*100 = 40%)

How many valence electrons does Cr have?

6

How many valence electrons does Sulfur have?

6

If a radioactive sample with an activity of 20 counts per minute has an activity of 1.25 counts per minute after 24 hours has passed, what is the half-life of this compound? 4 hours 6 hours 8 hours 12 hours

6 hours

After 18hrs 87.5% of a sample of a radioactive nuclide has decayed. What is its half-life? 36 hrs 54hrs 9hrs 6hrs

6hrs (Hint:After every half-life, only half of the sample remains. If 87.5% has decayed then 12.5% remains (100% - 87.5% = 12.5%) which is how much would remain after 3 half-lives: Latex Formula So 3 half-lives = 18hrs, therefore 1 half-life = 6hrs.)

How many valence electrons does Br have?

7

How many orbitals does the 3rd shell (n = 3) of an atom contain? 3 4 9 18

9 (Hint:The shortcut is that there are n2 orbitals in each shell. So the 3rd shell has 32 or 9 orbitals. Other than this you could have simply determined that the 3rd shell has 1 s orbital, 3 p orbitals, and 5 d orbitals for a total of 9.)

What is responsible for holding the Nucleus together? Strong Nuclear Force Electrostatic Repulsion Protons Nuclear Binding Energy B & C A & D

A & D (Hint: The Strong Nuclear Force holds the protons and neutrons together in the nucleus. The impact of this force is only seen when protons and neutrons are small distances apart. This distance is something observed inside the nucleus where the objects are tightly packed together. The strong force therefore overpowers the electrostatic repulsion force that you would typically observe from protons that are farther distances apart. Nuclear Binding Energy is simply the quantifiable energy required to split a nucleus.)

What is a Gamma Ray? A high-density nucleus particle A high-energy photon of light The heaviest form of radioactive decay in terms of AMU (mass unit) transfer A particle from the lowest part of the electromagnetic spectrum

A high-energy photon of light (Hint: Gamma Rays are high frequency forms of light. These photons of light (gamma rays) that are released during radioisotope decay are very light (much lighter than beta decay electrons) - almost massless. A gamma ray is a particle released and found within the highest end of the electromagnetic spectrum. Gamma rays are not high-density themselves (hence the fact they are almost massless) but they are actually absorbed best by high-density materials.)

What is a positron? A positively charged electron with the same mass and a spin of 1/2 A positron is a proton that is positiviely charged within the nucleus of an atom A positron is the result of electrostatic repulsion between different subatomic particles A positron is the opposite of a Neutron

A positively charged electron with the same mass and a spin of 1/2

Which of the following is paramagnetic? Cl- Ag Mg2+ Cu+

Ag (Hint:how many electrons each species has; if it has an odd number of electrons, then it must have unpaired electrons. Cl- has 18 electrons Ag has 47 electrons Mg2+ has 10 electrons Cu+ has 28 electrons. Ag is the only species with an odd number of electrons and must be the correct answer. Note that even though an odd number of electrons indicates the presence of unpaired electron(s), the converse isnt necessarily true. Just because a species has an even number of electrons doesnt mean it doesnt have any unpaired electrons. If every answer choice had an even number of electrons, further inspection of the electron configuration would have been required. In the ground state, all of the core electrons will be paired so we need only examine the valence electrons so it is convenient only to look at the noble gas configuration. Cl-: [Ar] Ag: [Kr]5s14d10 Mg2+: [Ne] Cu+: [Ar]3d10 Upon further inspection we can see silvers unpaired electron in the 5s orbital. We can also see that the other 3 species all have filled shells or subshells and therefore dont have any unpaired electrons.)

Based off these properties below, name the specific group from the periodic table. 1.) As they go down they get more reactive 2.) Form strong bases 3.) React explosively/violently with water

Alkali metals

Species whose ionic radius is larger than atomic radius.

Anions (Non-metal)

Quantum Numbers- Number: l What: Subshell (type of orbital) Range: [0...(n-1)] Name?

Azimuthal

When you are above the belt of stability you want to undergo _____ _____.

B decay

When your N/Z ratio is too high which route of decay do you undergo?

B decay

A nucleus emits an electron during which decay?

B-decay

Which of the following would have the highest 3rd ionization energy? Be B C N

Be (Hint: The 3rd ionization energy is the energy required to remove the 3rd electron. Beryllium is the only answer choice that has only 2 valence electrons (or fewer). Therefore the 3rd electron to remove is a core electron for beryllium and is much more difficult to remove than a valence electron. For all the other choices, the 3rd electron removed will still be a valence electron and therefore beryllium has the highest 3rd ionization energy.)

Which of the following result in the conversion of a proton into a neutron? Positron emission Beta decay Electron capture Both positron emission and electron capture

Both positron emission and electron capture

Which of the following has the highest (most negative) electron affinity? Be B C N

C (Hint: Electron affinities increase (get more negative) going left to right across a period but the groups (periods) containing Be and N are exceptions to the trend having either positive electron affinities or values close to zero. Therefore carbon has the highest (most negative) electron affinity rather than nitrogen. )

Which of the following is a network covalent solid? Rb2SO4 NH3 C(diamond) TiO2

C(diamond) (Hint: It should simply be remembered that the 2 very common examples of network covalent solids (also called simply network solids) are C(diamond) and SiO2 (quartz).)

Which of the following is the most polar bond? C-S C-O C-Br C-N

C-O

Which of the following compounds has the highest boiling point? CH3OH CH3CH2OH CH3CH2CH2F CH3CH2CH2OH

CH3CH2CH2OH (Hint: The compound with the highest intermolecular forces will have the highest boiling point. Typically we can rank intermolecular forces as follows: ionic or network covalent >> hydrogen bonding > dipole-dipole > London dispersion forces. Answer choice C is polar but is the only choice not capable of hydrogen bonding and so is eliminated. Choices A, B, and D all contain 1 O-H bond and therefore are capable of the same degree of H-bonding. But choice D is the largest (greatest surface area) of the 3 and therefore will have the greatest London dispersion forces and therefore the greatest overall intermolecular forces and the highest boiling point.)

Which of the following has the greatest intermolecular forces? CH4 CH3Cl CH2Cl2 CHCl3

CHCl3 (Hint: These 4 compounds are very different in molecular weight and therefore the determining factor will be molecular weight rather than polarity. CHCl3 is significantly heavier than the other 3 choices and will therefore have significantly greater London Dispersion forces than the other 3 and the greatest overall intermolecular forces.)

Rank these from smallest atomic radius to largest atomic radius. S 2-, Cl -, Ar, K +, Ca 2+

Ca 2+, K +, Ar, Cl -,S 2-

Have an ionic radius smaller than atomic radius.

Cation (Metal)

Which of the following has an ionic radius that is larger than its atomic radius? K Mg Ag Cl

Cl

Which of the following has the highest (most negative) electron affinity? Cl S P Si

Cl

Which of the following processes is exothermic? Sublimation Condensation Fusion Vaporization

Condensation

Which of the following is diamagnetic? Ca+ Mn2+ Fe3+ Cu+

Cu+ (Hint:An atom is diamagnetic if it contains no unpaired electrons. . The quick route here is to first see how many electrons each species has; if it has an odd number of electrons, then it must have unpaired electrons and can be eliminated. Ca+ has 19 electrons Mn2+ has 23 electrons Fe3+ has 23 electrons Cu+ has 28 electrons Cu+ is the only species which can be diamagnetic as the other 3 will have unpaired electrons having an odd number of electrons. Further inspection of the electron configuration of Cu+ confirms that it is indeed diamagnetic as all its shells and subshells are full. Cu+: [Ar]3d10)

_____-not attracted towards a magnetic field, all electrons are paired.

Diamagnetic

To what is an alpha particle equivalent in terms of mass and proton quantity? Equivalent to 1 AMU (mass) and 1 Proton Equivalent to 0 AMU (mass) and 0 proton and 1 electron Equivalent to Helium 4 AMU (mass) and 2 Protons Equivalent to 0 AMU (mass) and 1 Neutron

Equivalent to Helium 4 AMU (mass) and 2 Protons

Which of the following has the highest (most negative) electron affinity? C N O F

F

What is the most stable nucleus on the planet?

Fe (A=56)

Which of the following atoms are heaviest: Fe Fe^2+ Fe^1- They all weigh the same

Fe^1- (Answer: . This is heaviest because it has more electrons. As we have learned, that although electrons are NEARLY massless, they still have some mass. A good way to remember this is by realizing that in nuclear chemistry Beta decay and Positron emission produce a new product. In other words, that although we don't typically discuss the weight of an electron it is still there and causing changes to the radioactive reaction.)

Name four Halogens

Fluorine, Bromine, Iodine, Chlorine

Which particle has the most penetrating power? Alpha particle Positron Beta Particle Gamma Ray

Gamma Ray

Which of the following has the largest atomic radius? As Ge O S

Ge

Which of the following is the most polar bond? H-F H-Cl H-Br H-I

H-F

Which of the following has the greatest intermolecular forces? H2O H2S H2Se H2Te

H2O (Hint: Out of these 4 answer choices only H2O has hydrogen bonding and has the overall greatest intermolecular forces.)

Which of the following has the greatest intermolecular forces? H2S H2Se H2Te Cannot be determined without more information

H2Te (Hint: These 3 compounds are very different in molecular weight and therefore the determining factor will be molecular weight rather than polarity. H2Te is significantly heavier than the other 2 choices and will therefore have significantly greater London Dispersion forces than the other 2 and the greatest overall intermolecular forces.)

Which of the following elements has the highest vapor pressure? He Ne Ar Kr

He (Hint:The highest vapor pressure will be for the compound/element with the lowest intermolecular forces. These are all noble gases and are non-polar and therefore only have London dispersion forces. Helium is the smallest (and has the smallest surface area) and therefore has the lowest London dispersion forces and the highest vapor pressure.)

Which of the following is a property of ionic compounds? high melting points luster ductile malleable

High Melting Points (Hint: Ionic compounds tend to have higher melting and boiling points (there are a few more recently discovered exceptions). However, they are not malleable, ductile, or lustrous which are all properties of metals.)

Two atoms with the same atomic number but different mass numbers (different numbers of neutrons) are referred to as

Isotopes

Which of the following is an ionic compound? CO2 H3AsO4 KCl H2S

KCl

Which of the following is an ionic compound? CO2 H3AsO4 KCl H2S

KCl (Hint: An ionic compound is one composed of ions and is typically composed of either a metal and a nonmetal or of polyatomic ions. KCl is the only compound in the list composed of both a metal and nonmetal and is an ionic compound.)

Which of the following has an ionic radius that is smaller than its atomic radius? Li Cl O N

Li

Which of the following is not a property of metals? ductile malleable electrically conductive low melting points

Low Melting Points (Hint: The classic characteristic of metals is that they are malleable, ductile, electrically and thermally conductive, and typically have higher melting and boiling points (there are exceptions like mercury). But even though there are a handful of exceptions, it would definitely be false to say that metals of low melting points.)

How are mass (matter) and energy related or not related? Matter and Energy are related to each other because of the equation E=mc^2 . Matter and Energy are the same, except they are in two different forms. Matter and Energy are not related to each other because Energy is intangible and Matter is what makes up all inanimate and animate substances Matter and Energy are related because of the equation PV = nRT. Matter and Energy are the same, except they react different depending on temperature and pressure Matter and Energy are not related because they have no relative comparisons found in nature

Matter and Energy are related to each other because of the equation E=mc^2 . Matter and Energy are the same, except they are in two different forms. (Hint:In the Albert Einstein's equation - E = MC^2 it demonstrates if you convert mass into energy by multiplying the mass by the speed of light squared the resultant number would be the quantity of energy released from that mass. Keep in mind energy is neither created nor destroyed (Law of Conservation of Energy), thus indicating that matter and energy are related.)

Which of the following has the highest first ionization energy? B Cs C N

N

Which of the following has the highest first ionization energy? B C N O

N (Hint: 1st ionization energy increases going up a group (column) and to the right across a period (row) on the periodic table. But the answer choices here involve one of the exceptions to the general trend. Had this not been an exception we might have expected oxygen to be the correct answer. But the Group 5A elements (N, P, As) have higher 1st ionization energies than the Group 6A elements (O, S, Se) in the same period: N > O, P > S, and As > Se. The group 5A elements have electron configurations that end with s2p3. With the p subshell half-filled these tend to be more stable electron configurations thus explaining the higher energy required to remove an electron. (Its really a little more complex than this but this will suffice for any pre-health exam).

Which of the following is an ionic compound? NH4Br CO N2O4 SO2

NH4Br

Which of the following is an ionic compound? NH4Br CO N2O4 SO2

NH4Br (Hint: This one is a little tricky. Even though NH4Br is composed of all nonmetals it is still an ionic compound in that it contains a polyatomic ion (the ammonium ion). Ammonium salts should file away in your head as ionic compounds that are composed of all nonmetals.)

Which of the following would have the highest 2nd ionization energy? Na C Be Mg

Na (Hint: The 2nd ionization energy is the energy required to remove the 2nd electron. Sodium is the only answer choice that has only 1 valence electron (all the others have more than 1 valence electron). Therefore the 2nd electron to remove is a core electron for sodium and is much more difficult to remove than a valence electron.)

Which of the following has the highest boiling point? H2O CH3OCH3 NaCl HOCH2CH2OH Ar

NaCl (Hint: The compound with the highest intermolecular forces will have the highest boiling point. Typically we can rank intermolecular forces as follows: ionic or network covalent >> hydrogen bonding > dipole-dipole > London dispersion forces. NaCl is the only ionic compound listed among the answer choices and has a much higher boiling point than the other choices.)

Which of the following has the highest boiling point? HOCH2CH2OH CH3CH2OH NaOH H2O

NaOH (Hint:The compound with the highest intermolecular forces will have the highest boiling point. Typically we can rank intermolecular forces as follows: ionic or network covalent >> hydrogen bonding > dipole-dipole > London dispersion forces. NaOH is the only ionic compound listed among the answer choices and has a much higher boiling point than the other choices.)

Is this a possible set of quantum numbers in an atom? [3, 3, -1, +1/2]

No (Hint: l's maximum has to be 1 less than that n is)

Is this a possible set of quantum numbers in an atom? [3, 1, -2, -1/2]

No (Hint: l=1, ml could have been -1 or +1, but it cannot be -2)

Is this a possible set of quantum numbers in an atom? [3,2,-1, +1]

No (Hint: ms has to be + or - 1/2)

Which of the following is paramagnetic? O2- Cl- Li+ None of these

None of these

The strong nuclear force that holds protons together is also called _____ _____ _____.

Nuclear Binding Energy

What is the main distinguishing structural factor between nuclear chemistry and other general chemistry reactions? Nuclear chemistry deals with radiation Nuclear chemistry focuses on the nucleus and its components Nuclear chemistry focuses on electrons between transferred nuclei Nuclear chemistry focuses on heat energy being released

Nuclear chemistry focuses on the nucleus and its components (Hint: Nuclear chemistry focuses on the nucleus and its components encompasses the structural difference. General chemistry deals with reactions concerning the electrons surrounding the nucleus. Only in nuclear chemistry do we discuss the changes occurring to neutrons and protons by way of alpha, beta, and gamma decay or positron emission.)

Which of the following is a molecular compound? K2S MgCl2 PCl5 LiF

PCl5 (Hint: PCl5 is the only molecular compound listed, being composed of 2 nonmetals. K2S, MgCl2, and LiF are all ionic compounds, being composed of a metal and a nonmetal.)

An electron gets energy from _____ of light.

Photon

A positively charged electron is called a _____.

Positron

Rank from these least effective nuclear charge to most effective nuclear charge. S 2-, Cl -, Ar, K +, Ca 2+

S 2-, Cl-, Ar, K+, Ca 2+

Which of the following is diamagnetic? Cr3+ Cu2+ Sc3+ Mn2+

Sc3+

What is the molecular geometry of SF4?

See-saw

Quantum Numbers- Number: ml Name: Magnetic Range [-l...+l] What is this?

Specific orbital (orientation in space)

Which of the following has the largest atomic radius? P F Te S

Te (Hint: Atomic radius increases going down a group (column) and to the left across a period (row) on the periodic table. But the comparison here is challenging as phosphorus (P) is furthest to the left while tellurium (Te) is furthest down on the periodic table. The key is realizing that the increase in size in going down a group two periods is larger than going from right to left across a period one group, therefore Te (r = 140pm) has a larger atomic radius than P (phosphorus: r = 100pm). The increase down a group is easily explained by the increase in the number of shells of electrons. The increase from right to left across a period my seem a little counter-intuitive (since its opposite that of atomic mass) but is explained by the increase in effective nuclear charge experienced by the valence electrons as you go from left to right across a period. The greater effective nuclear charge results in the electrons being pulled closer to the nucleus and a smaller atomic radius.)

In Nuclear Chemistry are the reactants or products considered more stable? The reactants are more stable because they have not undergone radioactive decay and therefore are not radioactive The reactants are more stable because they have greater energy stored within their nuclei The products are more stable because they are now at a lower energy state, following the release of energy during radioactive decay The products are more stable because they are able to maintain a more controlled level radioactive decay

The products are more stable because they are now at a lower energy state, following the release of energy during radioactive decay (Hint: The reactants (parent elements) and the products (daughter elements) involved in nuclear chemistry are the key to understanding why radioactive decay moves forward. When reactants move forward during radioactive decay they release an incredible amount of energy. That energy thus moves the product down to a lower energy state. The product (daughter nuclei) is therefore far more stable, because the parent nuclei, upon reacting, has already released high amounts of energy.)

True or False: A nucleus always weighs a little bit less than all of its components.

True

hich of the following is a possible set of quantum numbers [n,l,ml,ms] for a valence electron in bromine? [4,0,0,-1/2] [3,1,1,+1/2] [4,1,-2,+1/2] [3,2,-1,-1/2]

[4,0,0,-1/2] (Hint:The electron configuration of Br is 1s22s22p63s23p64s23d104p5. The 4s and 4p electrons are considered the 7 valence electrons of Br and so the set of quantum numbers could describe an electron in either the 4s or 4p subshells. To be in the 4th shell, n=4 which eliminates choices B and D. To be in an s or p subshell, l=0 (s) or l=1 (p) so so far choices A or C could work. But ml is restricted in being an integer between l and +l. This rules out choice C as -2 is not between -1 and 1. That leaves choice A. Incidentally, ms can only have values of +1/2 or -1/2.)

Which of the following is a possible set of quantum numbers [n,l,ml,ms] for an electron? [3,3,0,-1/2] [3,2,1,-1] [5,0,0,-1/2] [4,1,2,+1/2]

[5,0,0,-1/2]

Which of the following could be a set of quantum numbers [n,l,ml,ms] for an electron in a 5f orbital? [5,4,0,-1/2] [5,3,4,+1/2] [4,3,-1,+1/2] [5,3,-1,-1/2]

[5,3,-1,-1/2] (Hint:The principal quantum number, n, describes the shell an electron is in and an electron in a 5f orbital is in the 5th shell so n = 5. Therefore all answers besides [5,4,0,-1/2], [5,3,4,+1/2] and [5,3,-1,-1/2] can be eliminated. The azimuthal quantum number, l, decribes what type of subshell (s, p, d, f) an electron lives in as follows: l=0 means s l=1 means p l=2 means d l= 3 means f Since the electron is in an f orbital, l=3. Therefore all answers besides [5,3,4,+1/2] and [5,3,-1,-1/2] can be eliminated. The magnetic quantum number, ml, takes on integer values from l to +l. Since in this case l=3, ml could either be -3, -2, -1, 0, +1, +2, or +3. This eliminates [5,3,4,+1/2] as 4 is not a possible value for ml in this case leaving [5,3,-1,-1/2] as the correct answer. But we can verify that ms is correct as well. The spin quantum number, ms, will always be either +1/2 or -1/2 for an electron and is -1/2 in the correct answer [4,1,-1,+1/2].)

What is the shorthand electron configuration for Cr 3+?

[Ar] 3d3

What is the shorthand electron configuration for Cr?

[Ar], 4s1, 3d5

What is the shorthand electron configuration for S?

[Ne], 3s2, 3p4

What is the shorthand electron configuration for S 2e-?

[Ne], 3s2, 3p6 or [Ne]

If your atomic number is higher than 83 what is your route of decay?

a-decay

Out of all the routes of decay which is the heaviest? Which is the lightest?

alpha particle, gamma ray

All atoms of a particular element will have the same _____ number, however they may differ in their number of _____ and _____.

atomic, neutrons, electrons

Which of the following is most likely to decay by beta emission? calcium-40 oxygen-16 carbon-14 nitrogen-14

carbon-14

Liquid----> Solid is called

crystallization

Azimuthal: l=2 Name the type of orbital

d orbital

_____ orbitals found in _____ subshells are four-lobed.

d, d

Which is more stable the parent nuclei or daughter? Which is lighter?

daughter, daughter

As you move to the left of the periodic table what happens to the atomic mass?

decreases

The atomic radius increases as you move _____ and to the _____ of the periodic table towards Fr.

down, left

An isoelectronic series all have the same number of _____.

electrons

An alpha decay is also sometimes called alpha _____.

emission

Is fusion exothermic or endothermic?

endothermic

As shells go further away from the nucleus, they increase in _____.

energy

Is deposition endothermic or exothermic?

exothermic

How many orbitals does shell number two have?

four (HINT: Every shell has n^2 orbitals, n=shell #)

Which of the following is most likely to be radioactive? oxygen-16 carbon-12 gold-196 magnesium-24

gold-196 (Hint:To look for likelihood of being radioactive, we should 1st look for odd numbers of protons and neutrons. If we cant come to a likely answer based upon this, then 2nd we could examine the N/Z ratios for elements with Z < 20. A significant deviation from a 1:1 ratio for an element with Z <20 would likely be radioactive. Oxygen-16: 8 protons, 8 neutrons Carbon-12: 6 protons, 6 neutrons Gold-196: 79 protons, 117 neutrons Magnesium-24: 12 protons, 12 neutrons Gold-196 has an odd number of both protons and neutrons and will in all likelihood be radioactive. No comparison of N/Z ratios is needed here.)

Which of the following is a property of ionic compounds? high melting points luster ductile malleable

high melting points

As you go across the periodic table from left to right the effective nuclear charge _____.

increases

What is the molecular geometry of HCN? trigonal planar tetrahedral bent linear

linear

Which of the following is not a property of metals? ductile malleable electrically conductive low melting points

low melting points

Paramagnetic- ion or element attracted towards a _____ _____. At least one _____ electron. The more you have the more paramagnetic you are going to be.

magnetic field, unpaired

The difference that has been converted into energy is called the _____ _____.

mass defect

Quantum Numbers- Name: spin, What: Up or down Range :+1/2 or - 1/2 Number?

ms

Which of the following electronic transitions in the hydrogen atom would involve an absorption of the highest energy photon? n=3 to n=5 n=1 to n=3 n=2 to n=4 n=5 to n=2

n=1 to n=3 (Hint: Photons are absorbed when an electron is promoted from a lower energy shell (lower principal quantum number) to a higher energy shell (higher principal quantum number) whereas the opposite (higher to lower) would correspond to the emission of a photon rather than the absorption. Therefore n=5 to n=2 would correspond to an emission of a photon (rather than an absorption) and is eliminated. The remaining three choices all involve a jump of two shells in energy but the gaps between energy levels are larger the lower in energy the shells and therefore the the largest jump in energy would be the transition from n=1 to n=3)

Which of the following electronic transitions in the hydrogen atom would involve an absorption a photon of the longest wavelength? n=1 to n=4 n=2 to n=3 n=4 to n=1 n=1 to n=3

n=2 to n=3 (Hint:Photons are absorbed when an electron is promoted from a lower energy shell (lower principal quantum number) to a higher energy shell (higher principal quantum number) whereas the opposite (higher to lower) would correspond to the emission of a photon rather than the absorption. Therefore n=4 to n=1 would correspond to an emission of a photon (rather than an absorption) and is eliminated. The key to choosing the correct answer from here is knowing that the energy and wavelength of a photon are indirectly proportional, so the lowest energy photon will have the longest wavelength. For the remaining three choices the smallest jump in energy (and longest wavelength photon) would be the transition from n=2 to n=3)

Which of the following electronic transitions in the hydrogen atom would involve an emission of a photon of the shortest wavelength? n=1 to n=5 n=3 to n=1 n=3 to n=2 n=5 to n=1

n=5 to n=1 (Hint:Photons are emitted when an electron is promoted from a higher energy shell (higher principal quantum number) to a lower energy shell (lower principal quantum number) whereas the opposite (lower to higher) would correspond to the absorption of a photon rather than the emission. Therefore n=1 to n=5 would correspond to an absorption of a photon (rather than an emission) and is eliminated. The key to choosing the correct answer from here is knowing that the energy and wavelength of a photon are indirectly proportional, so the highest energy photon will have the shortest wavelength. For the remaining three choices the largest drop in energy (and shortest wavelength photon) would be the transition from n=5 to n=1 )

Which of the following electronic transitions in the hydrogen atom would involve an emission a photon of the highest frequency? n=5 to n=2 n=2 to n=3 n=4 to n=3 n=1 to n=3

n=5 to n=2 (Hint:Photons are emitted when an electron is promoted from a higher energy shell (higher principal quantum number) to a lower energy shell (lower principal quantum number) whereas the opposite (lower to higher) would correspond to the absorption of a photon rather than the emission. Therefore n=1 to n=2 and n=2 to n=3 would correspond to an absorption of a photon (rather than an emission) and is eliminated. The key to choosing the correct answer from here is knowing that the energy and frequency of a photon are directly proportional, so the highest energy photon will have the highest frequency. )

Which has more energy, chemical reactions or nuclear reactions?

nuclear rxns

An alpha particle is an exact same thing as a Helium _____ but not the same thing as a Helium _____ because it has no _____.

nucleus, atom, electrons

Each subshell is further divided into _____. An _____ is defined as a region of space in which an _____ can be found. Only two electrons are possible per orbital. Thus, the s subshell may contain only _____ orbital and the p subshell may contain _____ orbitals.

orbitals, orbital, electron, one, three

_____ orbitals found in _____ subshells are two-lobed.

p, p

The heaviest route of decay (alpha particle) as the least _____ _____.

penetrating power

The lightest route of decay (amma ray) has the most _____ _____.

penetrating power

During _____ _____ and _____ _____ you are turning a proton into a neutron because your N/Z ratio is too low.

positron emission and electron capture

When you are below the belt you want to undergo _____ or _____.

positron emission or electron capture

Energy and frequency are _____. Energy, and frequency are_____ _____ to wavelength.

proportional, inversely proportional

Mass number, A, represents its number of _____ plus its number of _____.

protons, neutrons

Is electron capture a reactant or a product?

reactant

Azimuthal: l=0 Name the type of orbital

s orbital

There are four different types of subshells. These various types of subshells are denoted by the letters _____, _____, _____, and _____.

s, p, d, f

Each orbital has its own distinct shape. An _____ orbital found in a _____ subshell is spherical.

s, s

What is the hybridization of the central atom in XeF4? sp2 sp3 dsp3 sp3d2

sp3d2