practice Chemistry Periodic Trends Quiz
How many paired electrons does a neutral atom of Ir have in its 5d sublevel?
2
How many unpaired electrons will a Zr+2 ion have in its 4d sublevel?
2
How many unpaired electrons does an atom of Nb have?
3
How many unpaired electrons does an atom of Pd^+1 have?
3
How many unpaired electrons will a Co+2 ion have in its 3d sublevel?
3
How many paired electrons does a neutral Au atom have in its 5d sublevel?
4
How many unpaired electrons does an atom of Md^+3 have?
5
The electron configuration 1s2 2s2 2p6 represent all of the following except: a) K+ b) Mg+2 c) Ne0 d) F- e) Al+3
A (K+)
The elements in group 5A, as compared with those in group 4A, have: a) higher ionization energies, higher electronegativities & higher Zeff b) lower ionization energies, lower electronegativities & lower Zeff c) lower ionization energies, higher electronegativities & higher Zeff d) higher ionization energies, lower electronegativities & lower Zeff
A (higher ionization energies, higher electronegativities & higher Zeff)
The atoms of the most reactive metals have: a. large atomic radii and low ionization energies b. large atomic radii and high ionization energies c. small atomic radii and high ionization energies d. small atomic radii and low ionization energies
A (large atomic radii and low ionization energies)
An atom of calcium is larger than an atom of aluminum. One possible explanation is that calcium has: a) more electron shells b) a smaller atomic number c) a higher effective nuclear charge d) less unpaired electrons
A (more electron shells)
Which of the following depicts the electron configuration of an excited phosphorus atom? a) 1s2 2s2 2p6 3s2 3p3 b) 1s2 2s2 2p6 3s1 3p4 c) 1s2 2s2 2p6 3s2 3p2 d) 1s2 2s2 2p6 3s1 3p3
B (1s2 2s2 2p6 3s1 3p4)
Consider the following electron configurations: (a) 1s2, (b) 1s2 2s2 2p5, (c) 1s2 2s2 2p6, (d) 1s2 2s2 2p6 3s1 The atoms with the least reactivity will be: a) A and B b) A and C c) B and D d) C and D
B (A and C)
Which of the atom pairs both have only one unpaired electron? a) Se and Al b) Al and I c) K and Te d) I and Se
B (Al and I)
Consider the following electron configurations: (a) 1s2, (b) 1s2 2s2 2p5, (c) 1s2 2s2 2p6 3s1, (d) 1s2 2s2 2p6 3s2 The atoms with the most reactivity will be: a) A and B b) B and C c) C and D d) D and A
B (B and C)
Which of the following ions has a pseudo noble gas configuration? a) Ga+ b) In+3 c) Y+3 d) Cl- e) Se-2
B (In+3)
Which of the following groups of elements has similar chemical properties? a) O, S, Se, I, At, Ts b) Li, Na, K, Rb c) C, N, O, F d) B, Si, As, Te
B (Li, Na, K, Rb)
The electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 does not represent: a) Ti+2 b) Sc+3 c) Ca0 d) Cr+4 e) Fe+6
B (Sc+3)
Consider a neutral atom with the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d2. Which of the following is false? a) The element is Titanium b) The atom can lose 2 electrons to gain a pseudo-noble gas electron configuration c) The atom has 22 protons d) The element can lose 4 electrons to become stable e) The atom belongs to period 4
B (The atom can lose 2 electrons to gain a pseudo-noble gas electron configuration)
Which of the following statements about periodic trends is INCORRECT? a. Cations are smaller than the respective neutral atoms. b. Zeff stays same as we go across from left to right on the periodic table. c. Anions are larger than respective neutral atoms. d. As shielding increases, the ionization energy decreases.
B (Zeff stays same as we go across from left to right on the periodic table)
Which of the following is the most reactive metal? Ba, Be, Br, Bk
Ba
List the following elements in order of decreasing atomic radius: O, Mg, P, Ba, He
Ba, Mg, P, O, He
Which ground state electronic configuration will most readily produce a -1 ion? a) 1s2 2s22p6 b) 1s2 2s22p6 3s2 c) 1s2 2s22p6 3s23p5 d) 1s2 2s22p6 3s23p63d10 4s2 e) 1s2 2s22p6 3s23p63d10 4s24p6
C (1s2 2s22p6 3s23p5)
Which of the following groups of elements has similar chemical properties? a) Ti, Zr, Hf, Rf, La, Ac b) Rb, Sr, Y, Zr, Nb c) Cu, Ag, Au, Rg d) B, Si, Ge, As, Te
C (Cu, Ag, Au, Rg)
Which statement about periodicity is correct? a) Metal reactivity increases as atomic size decreases b) Non metal reactivity increases as IE decreases c) EN decreases as atomic size increases d) Z_eff changes within a group
C (EN decreases as atomic size increases)
Which of the following ions has an electronic configuration similar to Krypton? a) Se- b) Br-2 c) Rb+ d) Sr+
C (Rb+)
Which of the following reasons is incorrect for the decrease in electronegativity down a group: a) more electron shells b) valence electrons experience a weaker pull c) nuclear attraction increases on outer electrons d) Zeff stays constant
C (nuclear attraction increases on outer electrons)
The atoms of the most reactive non-metals have: a. large atomic radii and low ionization energies b. large atomic radii and high ionization energies c. small atomic radii and high ionization energies d. small atomic radii and low ionization energies
C (small atomic radii and high ionization energies)
What do the following have in common? Kr, Se-2, Rb+ a) They are isotopes of each other b) They are isomers of each other c) They are isoelectronic with each other d) They are different elements so they have nothing in common
C (they are isoelectronic with each other)
Which ionic species would you predict to be the smallest? P-3, Cl-, Ar0, Ca+2
Ca+2
Which of the following elements loses two electrons to gain a pseudo noble gas configuration? Co, Cr, Cl, Cd, Ca
Cd
Which ground state electronic configuration will most readily produce a +4 ion? a) 1s2 2s22p2 b) 1s2 2s22p6 3s2 c) 1s2 2s22p6 3s23p4 d) 1s2 2s22p6 3s23p63d4 4s2 e) 1s2 2s22p6 3s23p63d10 4s24p5
D (1s2 2s22p6 3s23p63d4 4s2)
Which of the following statements is incorrect? a) S-2 and Cl-1 are two examples of two nonmetallic ions that are iso-electronic with Ar b) Na+, Mg+2 and Al+3 three metallic ions that are iso-electronic with Ne c) Na, Mg and Al are in the third period and will be good conductors of heat. d) C, P & Se are soft shiny substances and can be cut with a knife
D (C, P & Se are soft shiny substances and can be cut with a knife)
Which of the atom pairs both have four unpaired electrons in their f sublevel? a) Mo and Es b) Es and Os c) Mo and Os d) Es and Nd
D (Es and Nd)
In which set are all atoms/species isoelectronic? a) S-2, K0, Ca+1 b) Ga+, Al+, In+ c) K+, Kr0, Br- d) I-, Xe0, Cs+ e) Ne0, Li+, Be+2
D (I-, Xe0, Cs+)
Which of the following atoms has the smallest number of unpaired electrons? a) Nb b) Es c) Se d) Na e) Ir
D (Na)
Which pair of elements would most readily form an ionic compound? a) Mg, O b) Li, Se c) Ba, Cl d) Na, I e) Cs, O
D (Na, I)
Which statement about periodicity is incorrect? a) Ionization energy increases as atomic size decreases b) Electronegativity decreases as number of energy levels increase c) Metals with low IE are more reactive d) Non-metals with low electronegativity are more reactive
D (Non-metals with low electronegativity are more reactive)
Which of the following atoms has the greatest number of unpaired electrons? a) F b) Zr c) Pd d) Pu e) Ba
D (Pu)
In which set do the atoms/species have different numbers of electrons? a) O-2, F-1, Ne0 b) Rn0, Po-2, Fr+ c) K+, Ca+2, Sc+3 d) S-2, K0, Ca+1 e) none of these
D (S-2, K0, Ca+1)
Consider a neutral atom with the electron configuration 1s2 2s2 2p6 3s2 3p4. Which of the following is true? a) The element most likely forms +2 ions b) The element's atomic number 18 c) The 2p and 3p orbitals are filled d) The element's symbol is "S" e) The element is a halogen
D (The element's symbol is "S")
Which of the following ions does not have a pseudo noble gas configuration? a) Pb+4 b) In+3 c) Zn+2 d) Ti+4
D (Ti+4)
Which of the following reasons is incorrect for increase in metal reactivity down a group: a. atomic size increase as energy levels increase b. nuclear attraction decreases on outer electrons c. valence electrons experience a weaker pull d. Zeff increases
D (Zeff increases)
Sulfur has a higher electronegativity than strontium. A possible explanation is that compared to strontium sulfur has: a) a lower ionization energy b) a smaller nuclear charge c) more unpaired electrons d) a smaller atomic radius
D (a smaller atomic radius)
Which of the following is NOT true about atomic & ionic radii? a. ionic radius of a cation is less than the atomic radius of the neutral metal atom b. ionic radius of a anion is more than the atomic radius of the neutral non metal atom c. atomic radii increases down the group d. atomic radius increases across the period
D (atomic radius increases across the period)
The elements in group 2A, as compared with those in group 3A, have: a) higher atomic radius, higher electronegativities & higher IEs b) lower atomic radius, higher electronegativities & lower IEs c) lower atomic radius, lower electronegativities & lower IEs d) higher atomic radius, lower electronegativities & lower IEs
D (higher atomic radius, lower electronegativities & lower IEs)
Which of the following is a property of halogens? a) form +1 cations b) have one more electron than the next noble gas c) show a gradual increase in electronegativity d) react with metals
D (react with metals)
What do the following have in common? He, H-, Li+ a) They are isotopes of each other b) They are belong to the same period c) They are all electronically similar to an isosceles triangle d) They have the same number of electrons
D (they have the same number of electrons)
Which of the following configurations depicts an excited krypton atom? a) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 b) 1s2 2s2 2p6 3s2 3p6 4s2 3d11 4p5 c) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 d) 1s2 2s2 2p6 3s2 3p6 4s1 3d10 4p7 e) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 5s1
E (1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 5s1)
The electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d7 represents: a) Mn0 b) Y+ c) Ti+2 d) Fe+ e) Co0
E (Co0)
Which pair of elements would be least likely to form an ionic compound? a) Be, I b) Na, Cl c) K, F d) Li, I e) O, C
E (O, C)
Whic hstatement about the relationship between periodic trends is INCORRECT a. As atomic radius increases the ionization energy of metals decrease. b. As electronegativity of non metals decrease, the non metal reactivity also decreases. c. Cations are smaller than its metal atom & Anions are larger than its non metal atom. d. Lower ionization energy indicated higher metal reactivity. e. none of the above
E (none of the above)
Which of the following ions has an electronic configuration similar to calcium? a) Ti+2 b) K+ c) Sc+3 d) Ga+ e) none of the above
E (none of the above)
Alkaline earth metals have all of the following properties except: a) have 2 electrons in the valence shell b) readily form cations c) form +2 ions d) show a gradual increase in atomic radius e) show a gradual increase in IE
E (show a gradual increase in IE)
List the following from greatest to least electronegativity: Mg, F, Cs
F, Mg, Cs
Rank the following five atomic species in order of increasing atomic radius: Si, Na, K, F, O
F, O, Si, Na, K
True/False: Se has an electron configuration ending in 3p4. If false, what is the correction?
False - 4p4
Which element has the highest electronegativity?
Fluorine
What is the most reactive metal?
Fr
Which element has the largest atomic radius?
Francium
Which element has the highest first ionization energy?
Helium
Rank the following atoms in order of decreasing atomic radius: Si, Cl, K, Ca, Ga
K, Ca, Ga, Si, Cl
Which of the following is not a monoatomic ion? Sr+2, S-2, Li+, KS-, N-3
KS-
Which element has an electron configuration ending in 5f3?
Pa
Which of the following has the largest second IE compared to its first IE? Rb, Nb, Sb, Pb, Tb
Rb
Which ionic species would you predict to be the largest? Se-2, Br-, Rb+, Sr+2
Se-2
Identify the element with a 5p2 configuration for its last electron
Sn
Which of the following has the smallest second IE compared to its first IE? S, Se, Sb, Sr, Si
Sr
List the following from least to greatest electronegativity: Se, Sr, O
Sr, Se, O
Which of the following elements does not form a pseudo noble gas configuration by losing 2 or 3 electrons? Hg, V, Ga, In
V
Write the core electron configuration of a ground-state Ru atom
[Kr] 5s2 4d6
Write the core electron configuration of a ground-state P atom
[Ne] 3s2 3p3
