chemistry chapter 8

How many electrons are in the 4p subshell of vanadium? A) 0 B) 2 C) 4 D) 5 E) 6

A) 0

Which of the following elements is found as a monatomic species in its most stable form? A) sulfur B) oxygen C) hydrogen D) argon E) phosphorus

All the noble gases are monatomic species; thus we use their symbols: He, Ne, Ar, Kr, Xe, and Rn D) argon

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) ® Hg+(g) + e- is therefore A) 1006 kJ/mol. B) greater than 1006 kJ/mol. C) less than 1006 kJ/mol. D) is equal to the electron affinity of mercury. E) is equal to the second ionization energy of mercury.

B) greater than 1006 kJ/mol.

section 8.6 The elements in Group 7A are known by what name? A) transition metals D) alkaline earth metals B) halogens E) noble gases C) alkali metals

B) halogens

Which of the following elements is found as a monatomic species in its most stable form? A) nitrogen B) neon C) sulfur D) chlorine E) fluorine

B) neon

Which of the following is the general electron configuration for the outermost electrons of the elements in Group 5A?

D) ns2np3 see page 355

Concerning the electron configuration of fluorine, 1s22s22p5 which of the following represents the core electrons only? A) 1s2 B) 1s22s2 C) 1s22s22p5 D) 2s22p5 E) 2p5

A) 1s2 F 9 electrons 5p+2s=7 9-7 =2 1s2

Which one of the following elements forms a stable 3- anion? A) P B) S C) Cl D) Al E) Mg

A) P see pg 335 but P has a -3

How many valence electrons does P3- have? A) 3 B) 8 C) 15 D) 1 E) 18

B) 8

How many core electrons does a silicon atom have? A) 14 B) 10 C) 4 D) 8 E) 2

B) 10

Which two electron configurations represent elements that would have similar chemical properties? (1) 1s22s22p4 (2) 1s22s22p5 (3) [Ar]4s23d5 (4) [Ar]4s23d104p5 A) (1) and (2) B) (1) and (3) C) (2) and (3) D) (2) and (4) E) (3) and (4)

D) (2) and (4)

How many electrons does a bromine atom need to fill its outermost s and p subshells? A) 8 B) 7 C) 5 D) 3 E) 1

E) 1

Since arsenic is a nonmetal, As2O3 is expected to be a/an _____ oxide. A) acidic B) ionic C) amphoteric D) neutral E) basic

A) acidic

Which of the following elements behaves chemically similarly to oxygen? A) magnesium B) sodium C) sulfur D) chlorine E) iron F) beryllium

sulfur D)

What are the products of the following reaction? SO2(g) + H2O(l) ----> A) H2SO4(aq) D) S(s) + H2O(l) B) H2SO3(aq) E) S(s) + H2(g) + O2(g) C) H2(g) + SO3(g)

B) H2SO3(aq) pg 356

Section: 8.1 The law of octaves was proposed by A) G. N. Lewis. D) J. J. Thompson. B) John Newlands. E) Ernest Rutherford. C) Dmitri Mendeleev

B) John Newlands.

Which of the atoms listed below has the smallest radius? A) Al B) P C) As D) Te E) Na

B) P see chart

Which of the following is the electron configuration of a sulfide ion? A) [Ne]3s23p4 B) [Ne] C) [Ne]3s23p1 D) [Ar] E) [Ne]3s23p2

D) [Ar] sulfide =S^2- =18 electrons

Which of the following is the electron configuration for the bromide ion? A) [Ar] B) [Ar]4s23d104p7 C) [Kr] D) [Kr]5s24d105p7 E) [Xe]

D) [Kr] bromide=36 electrons

The elements in Group 2A are known by what name? A) transition metals D) alkaline earth metals B) halogens E) noble gases C) alkali metals

D) alkaline earth metals

The alkali metal elements are found in _______ of the periodic table. A) Group 1A B) Group 2A C) Group 3A D) Period 7 E) Period 1

A) Group 1A

Which of the elements listed below has the highest first ionization energy? A) He B) Ne C) Ar D) Kr E) Xe

A) He see pg 344 The increase in first ionization energy from left to right across a period and from bottom to top in a group for representative elements.

Arrange the following ions in order of increasing ionic radius: K+, P3- , S2-, Cl-. increasing radius ® A) K+ < Cl- < S2- < P3- D) Cl- < S2- < P3- < K+ B) K+ < P3- < S2- < Cl- E) Cl- < S2- < K+ < P3- C) P3- < S2- < Cl- < K

A) K+ < Cl- < S2- < P3-

Consider the element with the electron configuration [Kr]5s24d105p5. This element is A) a representative element D) an actinide element B) a transition metal E) a noble gas C) an alkali metal

A) a representative element The Groups or Families can be further categorized into the Representative Elements and the Transition Metals. The Representative Elements are those elements within the first two families (Groups I and II on the far left) and the last six families or groups (on the right) of the Periodic Table. The Transition Metals are the elements in those Groups within the middle of the Table.

Which of the following elements is found as a diatomic species in its most stable form? A) bromine B) neon C) sulfur D) xenon E) phosphorus

A) bromine hydrogen, nitrogen, oxygen, and the halogens exist as diatomic molecules 7 diatomics are Hydrogen (H2) Nitrogen (N2) Oxygen (O2) Fluorine (F2) Chlorine (Cl2) Iodine (I2) Bromine (Br2)

An element with the general electron configuration for its outermost electrons of ns2np1 would be in which element group?

B) 3A Group 3A Elements (ns2np1, n ≥ 2)

Which of the elements listed below has the greatest atomic radius? A) B B) Al C) S D) P E) Si

B) Al

Which of the following elements has the greatest electron affinity (largest positive value)? A) K B) Br C) As D) Ar E) I

B) Br

Which of the following is a basic oxide? A) CO2 B) CaO C) SO2 D) H2O E) NO2

B) CaO The first two oxides of the third period, Na2O and MgO, are basic oxides

section 8.2 Which one of the following elements is a Lanthanide? A) U B) Ce C) Os D) Bi E) Cs

B) Ce The lanthanides and actinides are sometimes called f-block transition elements because they have incompletely filled f subshells

Which of the elements listed below has the smallest first ionization energy? A) C B) Ge C) P D) O E) Se

B) Ge

Which of the following is a basic oxide? A) CO2 B) MgO C) As2O3 D) SO2 E) Cl2O7

B) MgO

Which of the following elements behaves chemically similarly to potassium? A) magnesium B) sodium C) beryllium D) chlorine E) iron

B) sodium

The electron affinity of fluorine is essentially equal to A) the negative of the ionization energy F. B) the ionization energy F-. C) the negative of the ionization energy F-. D) the ionization energy Ne. E) the negative of the ionization energy Ne.

B) the ionization energy F-.

Concerning the electron configuration of sulfur, 1s22s22p63s23p4, which of the following represents the core electrons only? A) 1s2 B) 1s22s2 C) 1s22s22p6 D) 1s22s22p63s2 E) 3s23p4

C) 1s22s22p6 S=16 4p+2s=6 16-6=10 C) 1s22s22p6

What are the products of the following reaction? 2 Li(s) + 2H2O(l) ----> A) Li2O2(s) + 2 H2(g) D) 2 Li(s) + 2H2O(l) B) 2Li2O(s) + 2 H2(g) E) LiO2(s) + 2H2(g) C) 2 LiOH(aq) + H2(g)

C) 2 LiOH(aq) + H2(g)

How many core electrons does a chlorine atom have? A) 17 B) 7 C) 10 D) 18 E) 8

C)10 the total number of electrons is the same as the atomic number, for Cl 17 its in notice that Sn is in the part of the table (columns 13-18) where the p-orbitals are filling (since it's in the 5th column, it has 5 valence electrons in the p orbitals). If p-oritals are filling, then the s-orbitals are already full (add 2 more valence electrons). Therefore you have 7 total.17-7=10 core electrons

isoelectronic

Ca^2+<K^+<Cl-<S^2-<P^3-

Which of the following is the electron configuration for the aluminum ion? A) 1s22s22p63s2 D) 1s22s22p6 B) 1s22s22p63s23p2 E) 1s22s22p63s23p4 C) 1s22s22p63s23p

D) 1s22s22p6 Al^3+= 13+3=16 electrons

How many electrons does a sulfur atom need to fill its outermost s and p subshells? A) 6 B) 8 C) 4 D) 2 E) 1

D) 2 (count the the spaces to the right) ONIZATION ENERGY (or FIRST IONIZATION ENERGY) - The amount of energy required to remove a single electron from the outer shell of an atom. - As you go DOWN A GROUP ( ), the ionization energy DECREASES. - Relates to reactivity for metals. The easier it is to remove an electron, the more reactive the metal. - Why? As you go down a period, you are ADDING SHELLS. Since the outer electrons are farther friom the nucleus and charge attraction lessens with distance, this makes electrons easier to remove as the atoms get bigger! - As you go ACROSS A PERIOD ( ), the ionization energy INCREASES. http://scienceattech.com/wp-content/uploads/2010/04/c100z-042610a.pdf

What are the products of the following reaction? H2(g) + Cl2(g) ---> A) H2O(l) + 2HCl(g) D) 2HCl(g) B) H2(g) + Cl2(g) E) HCl2(g) + H+(aq) C) H2Cl(g) + Cl-(aq)

D) 2HCl(g)

What are the products of the following reaction? CaH2(s) + 2H2O(l) --->

D) Ca(OH)2(s) + 2H2(g) see pg 350 Hydrogen (1s1)

Which of the following make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+? A) Ca2+ and Fe3+ D) Cl- and Ca2+ B) O2- and F E) None of the above. C) F and Cl-

D) Cl- and Ca2+ Ions, or atoms and ions, that possess the same number of electrons Cl-=18 Ca2+=18

The law of octaves states that every eighth element has similar properties when arranged in order of increasing A) nuclear binding energy. D) atomic mass. B) number of electrons. E) atomic number. C) number of neutrons.

D) atomic mass

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing A) nuclear binding energy. D) atomic number. B) number of neutrons. E) atomic size. C) atomic mass.

D) atomic number.

Concerning the electron configuration of aluminum, 1s22s22p63s23p1, which of the following represents the valence electrons only? A) 1s2 B) 1s22s2 C) 1s22s22p6 D) 1s22s22p63s2 E) 3s23p1

E) 3s23p1 2s+1p=3

How many valence electrons does S2- have? A) 2 B) 4 C) 6 D) 16 E) 8

E) 8 valance electrons can be found in the highest energy levels of the S and P sublevels 1s2,2s2,2ps,3s2,4p6 6+2=8 valance electrons

Which of the following elements has the greatest metallic character? A) Br B) F C) Ge D) Mn E) Sc

the metallic character increases from top to bottom. Most beryllium compounds (BeH2 and beryllium halides, such as BeCl2) and some magnesium compounds (MgH2, for example) are molecular rather than ionic in nature.

How many electrons does a nitrogen atom need to fill its outermost s and p subshells? A) 5 B) 3 C) 1 D) 8 E) 0

B) 3

Which of the following elements behaves chemically similarly to calcium? A) magnesium B) sodium C) sulfur D) chlorine E) iron

A) magnesium

Which of the following is the general electron configuration for the outermost electrons of the noble gases? A) ns2np6 B) ns2np5 C) ns2np4 D) ns2np3 E) ns2

A) ns2np6 Group 8A Elements (ns2np6, n ≥ 2)

Which of the following is the electron configuration of the iron(III) ion? A) [Ar]3d5 B) [Ar]4s13d5 C) [Ar]4s23d3 D) [Ar]3d6 E) [Ar]4s23d9

A) [Ar]3d5

Mendeleev proposed the existence of an unknown element that he called eka-aluminum. This element is now called A) gallium. B) silicon. C) magnesium. D) boron. E) germanium

A) gallium.

What are the products of the following reaction? 2Al(s) + 6H+(aq) ----> A) 2Al3+(aq) + 3H2(g) D) 2Al+(aq) + 3H2(g) B) 2Al2+(aq) + 3H2(g) E) 2AlH3(s) C) 2AlH2(s) + H2(g)

A) 2Al3+(aq) + 3H2(g)

Consider the following reaction 2A + 3F2 --> 2AF3. What is the formula for the reaction product if we substitute sulfur for fluorine? A) A2S3 B) A3S2 C) AS3 D) A3S E) AS

A) A2S3

Which one of the following is not isoelectronic with Kr? A) As3+ B) Se2- C) Rb+ D) Sr2+ E) Br-

A) As3+

Which of the following is an acidic oxide

A) P4O10 acidic oxide are two nonmetal

For which of the following reactions is the enthalpy change equal to the third ionization energy of vanadium? A) V2+(g) ® V3+(g) + e- D) V2-(g) + e- ® V3-(g) B) V3+(g) + e- ® V2+(g) E) V3+(g) ® V4+(g) + e- C) V(g) ® V3+(g) + 3e-

A) V2+(g) ® V3+(g) + e- D) see pg 343 for the second ionization energy (IE2) and the third ionization energy (IE3)

Consider the element with the electron configuration [Xe]6s24f7. This element is A) a representative element D) an actinide element B) a lanthanide element E) a noble gas C) a nonmetal

B) a lanthanide element

Consider the element with the electron configuration [Kr]5s^24d^7. This element is A) a representative element. D) an actinide element. B) a transition metal. E) a noble gas. C) a nonmetal

B) a transition metal.

The representative elements are those with unfilled energy levels in which the "last electron" was added to A) an s orbital. D) a p or d orbital. B) an s or p orbital. E) an f orbital. C) a d orbital.

B) an s or p orbital

Which of the following elements behaves chemically similarly to silver? A) nickel B) gold C) sulfur D) chlorine E) iron F) beryllium

B) gold

Which of the following is the general electron configuration for the outermost electrons of elements in the alkaline earth group?

B) ns2 Group 2A Elements (ns2, n ≥ 2)

Which of the following is the general electron configuration for the outermost electrons of the halogens? A) ns2np6 B) ns2np5 C) ns2np6(n -1)d7 D) ns1 E) ns2np

B) ns2np5 Group 7A Elements (ns2np5, n ≥ 2)

How many electrons are in the 4p subshell of selenium? A) 0 B) 2 C) 4 D) 5 E) 6

C) 4

Which of the following reactants can be combined to produce a basic oxide as a product? A) Cl2O7(l) + H2O(l) ® D) Al2O3(s) + 6HCl(aq) ® B) P4O10(s) + 6H2O(l) ® E) MgO(s) + 2HCl(aq) ® C) 4Li(s) + O2(g) ®

C) 4Li(s) + O2(g) ---> Lithium forms lithium oxide (containing the O2− ion):

Consider the following reaction 2A + 3F2 -->2AF3. What is the formula for the reaction product if we substitute iodine for fluorine?

C) AI3

Which of the following is an amphoteric oxide? A) Na2O B) MgO C) Al2O3 D) SO2 E) Cl2O7

C) Al2O3 Al2O3 is classified as an amphoteric oxide because it has properties of both acids and bases. Other amphoteric oxides are ZnO, BeO, and Bi2O3.

Which of the following elements has the greatest metallic character? A) Ca B) Mg C) Ba D) As E) Se

C) Ba

Which of the following is a basic oxide? A) NO2 B) H2O C) Na2O D) SnO E) SO2

C) Na2O

Which of the following elements has the greatest metallic character? A) Br B) Se C) Ni D) As E) Si

C) Ni

Which one of the following ions has the largest radius? A) Cl- B) K+ C) S2- D) Na+ E) O2-

C) S2-

If the radius of atom X is greater than the radius of atom Y, then it is also likely that A) X has a larger electron affinity than Y does. B) X has a larger effective nuclear charge than Y does. C) X has greater metallic character than Y does. D) X has a larger first ionization energy than Y does. E) X is a poorer conductor of electricity than Y when in the solid state

C) X has greater metallic character than Y does

In a surprisingly large number of their properties, beryllium resembles aluminum and boron resembles silicon. Such a relationship is called A) amphoterism. D) the periodic law. B) an allotropic relationship. E) an isoelectronic series. C) a diagonal relationship.

C) a diagonal relationship.

Which one of the following elements is a transition element? A) antimony B) barium C) chromium D) potassium E) selenium

C) chromium

The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s) ® Na+(g) + e- is therefore A) 495.9 kJ/mol. B) less than 495.9 kJ/mol. C) greater than 495.9 kJ/mol. D) is equal to the electron affinity of sodium. E) is equal to the second ionization energy of sodium.

C) greater than 495.9 kJ/mol.

The second ionization energy of Mg is ________ than its first ionization energy, and is __________ than the second ionization energy of Na. A) higher, higher B) lower, higher C) higher, lower D) lower, lower

C) higher, lower

In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s24d105p2? A) row 4, group 4A D) row 5, group 5A B) row 4, group 5A E) none of the above C) row 5, group 4A

C) row 5, group 4A

The chief contribution of physicist Henry Moseley to atomic theory was A) the discovery of the periodic law. B) the determination of the charge of the proton. C) the measurement of the atomic numbers of the elements. D) the scientist who determined the electric charge of the electron. E) the discovery of the law of octaves

C) the measurement of the atomic numbers of the elements.

Which of the following elements has the smallest first ionization energy? A) Cl B) Na C) Be D) K E) As

D) K

Which of the following reactants can be combined to produce hydrogen gas as a product? A) N2O5(s) + H2O(l) D) Mg(s) + 2H+(aq) ® B) H2(g) + Cl2(g) ® E) 2H2(g) + O2(g) ® C) 2 F2(g) + 2H2O(l) ®

D) Mg(s) + 2H+(aq) --->

section 8.4 For which of the following reactions is the enthalpy change equal to the second ionization energy of nitrogen? A) N2+= N3+(g) + e- D) N-(g) + e- = N2-(g) B) N2+(g) + e- = N+(g) E) N+(g) = N2+(g) + e- C) N(g) =N2+(g) + 2e-

D) N-(g) + e- = N2-(g) see pg 343 for the second ionization energy (IE2) and the third ionization energy (IE3)

Consider the following reaction: 3Li + Z -->Li3Z. What is the formula for the compound if we substitute sodium for lithium? A) NaZ B) Na2Z C) NaZ2 D) Na3Z E) NaZ3

D) Na3Z

Which of the elements listed below has the highest first ionization energy? A) C B) Ge C) P D) O E) Se

D) O

Which of the atoms listed below has the largest radius? A) Cl B) I C) P D) Sb E) Se

D) Sb

Which one of the following elements forms a stable 2+ cation? A) Kr B) I C) Se D) Al E) Ba

E) Ba

Which pair of elements from different groups resemble each other the most in their chemical properties? A) Be and B B) Al and Si C) Li and Be D) Al and Be E) Be and C

E) Be and C see Figure 8.13

Which of the following atoms has the greatest electron affinity (largest positive value)? A) S B) P C) Ga D) Li E) Br

E) Br

Which ion is isoelectronic with Ar? A) Fe2+ B) F- C) Br- D) Ga3+ E) Ca2+

E) Ca2+

The effective nuclear charge (Zeff) felt by the outermost electrons is the strongest for which of the following elements? A) Al B) Si C) P D) S E) Cl

E) Cl which ever element is closets to the right

8.3 The effective nuclear charge (Zeff) felt by the outermost electrons is the strongest for which of the following elements? A) B B) C C) N D) O E) F

E) F which ever element is closets to the right

Which one of the following elements forms a stable 1- anion? A) K B) Be C) Al D) O E) I

E) I

Which one of the following pairs are isoelectronic? A) Mn2+ and Ar D) Cl- and S B) Zn2+ and Cu2+ E) K+ and Cl- C) Na+ and K+

E) K+ and Cl- K+-18 Cl-=18

Consider the following reaction: 3Li + Z --> Li3Z. What is the formula for the compound if we substitute magnesium for lithium?

E) Mg3Z2

Arrange the following ions in order of decreasing ionic radius: Al3+, Mg2+, Na+, O2-. decreasing radius ® A) Al3+ > Mg2+ > O2- > Na+ D) O2- > Al3+ > Mg2+ > Na+ B) Al3+ > Mg2+ > Na+ > O2- E) O2- > Na+ > Mg2+ > Al3+ C) Na+ > Mg2+ > Al3+ > O2-

E) O2- > Na+ > Mg2+ > Al3+

Which of the following elements has the smallest ionization energy? A) Li B) Na C) Be D) K E) Rb

E) Rb

Which of the following elements has the greatest electron affinity (largest positive value)? A) Mg B) Al C) Si D) P E) S

E) S

Which one of the following is not isoelectronic with the others: Br-, Rb+, Se2-, Sr2+, Te2-? A) Br- B) Rb+ C) Se2- D) Sr2+ E) Te2-

E) Te^2-

Since zirconium is a metal, ZrO2 is expected to be a/an _____ oxide. A) acidic B) ionic C) amphoteric D) neutral E) basic

E) basic Most oxides can be classified as acidic or basic depending on whether they produce acids or bases when dissolved in water or react as acids or bases in certain processes