Periodic Table
Which of the following Group 15 elements has the most metallic properties? a) Bi b) P c) Sb d) N
a) Bi
Which halogen is liquid at STP? a) Br₂ b) F₂ c) Cl₂ d) I₂
a) Br₂
An atom of which element in the ground state has a complete outermost energy level? a) He b) Be c) Hg d) H
a) He
Which element attains the structure of a noble gas when it becomes a 1+ ion? a) K b) Ca c) F d) Ne
a) K
which elements have the most similar chemical properties? a) K and Na b) K and Cl c) K and Ca d) K and S
a) K and Na
Which group below contains elements with the greatest variation in chemical properties? a) Li, Be, B b) Li, Na, K c) B, Al, Ga d) Be, Mg, Ca
a) Li, Be, B
The diagram below represents atoms of two unknown elements (X and Z) undergoing a reaction. ⃝+⃝→⃝ +⃝ X Z X+ Z- a) Which particle (X or Z) most likely represents a metal atom? [Give one reason to support your answer.] b) Which particles (X or Z) most likely represents a nonmetal atom? [Give one reason to support your answer.]
a) X gets smaller b) Z gained electrons and got bigger
If X represents an element of Group 1 (1A), the formula of its oxide would be a) X₂O b) X₂O₃ c) XO d) XO₂
a) X₂O
An element that has a high ionization energy and tends to be chemically inactive would most likely be a) a noble gas b) an alkali metal c) a transition element d) a halogen
a) a noble gas
Which halogens are gases at room temperature and pressure? a) chlorine and fluorine b) chlorine and bromine c) iodine and fluorine d) iodine and bromine
a) chlorine and fluorine
As the elements of Group 1 are considered in order from top to bottom, the first ionization energy of each successive element will a) decrease b) increase c) remain the same d) follow an unpredictable pattern
a) decrease
As atoms of elements in Group 16 are considered in order from top to bottom, the electronegativity of each successive element a) decreases b) increases c) remains the same
a) decreases
Within Period 2 of the periodic table, as the atomic number increases, the atomic radius generally a) decreases b) increases c) remains the same d) follows no pattern
a) decreases
Which statement describes a chemical properly of the element iodine? a) it reacts with hydrogen to form a gas b) it forms a violet-colored gas c) it dissolves in alcohol d) its crystals are a metallic gray
a) it reacts with hydrogen to form a gas
Which atom in the ground state has a stable electron configuration? a) neon b) carbon c) magnesium d) oxygen
a) neon
According to the reference table, which of the following elements has the smallest radius? a) nickel b) cobalt c) calcium d) potassium
a) nickel
Which Group 15 element exists as a diatomic molecule at room temperature and pressure? a) phosphorus b) nitrogen c) bismuth d) arsenic
b) nitrogen
Choose two elements from the list below which would have the most similar chemical properties. Explain why. Na, Ni, Mg, Ba, B
Mg & Ba They are in the same group and same number valance of electrons.
Sodium and cesium are both elements in Group 1. They have the same number of valence electrons and similar chemical properties. For example, they both explode in water. however, cesium reacts more violently in water than sodium. explain why cesium is more reactive than sodium.
Because cesium has a low ionization energy.
Which of the following groups in the periodic table contain elements so reactive that they are never found in the free state? a) 1 and 2 b) 1 and 11 c) 2 and 15 d) 11 and 15
a) 1 and 2
Which group is represented by the electron dot symbol ∙Ẍ:͘ ͘͘͘ ∙ a) 16 (VIA) b) 14 (IVA) c) 17 (VIIA) d) 15 (VA)
a) 16 (VIA)
Which element in Group 15 has the strongest metallic character? a) Bi b) As c) P d) N
a) Bi
A diatomic element with a high first ionization energy would most likely be a a) nonmetal with a high electronegativity b) nonmetal with a low electronegativity c) metal with a high electronegativity d) metal with a low electronegativity
a) nonmetal with a high electronegativity
As the elements are considered from top to the bottom of Group 15, which sequence in properties occurs? a) nonmetals → metalloid → metal b) metal → metalloid → nonmetal c) metal → nonmetal → metalloid d) metalloid → metal → nonmetal
a) nonmetals → metalloid → metal
As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? a) nonmetals→metalloid→metal b) metalloid→metal→nonmetal c) metal→metalloid→nonmetal d) metal→nonmetal→metalloid
a) nonmetals→metalloid→metal
Which element is more reactive than strontium? a) potassium b) calcium c) iron d) copper
a) potassium
In which section of the period table are the most active nonmetals located? a) upper right corner b) lower right corner c) upper left corner d) lower left corner
a) upper right corner
Which group is known as the halogens? a) 2 (IIA) b) 17 (VIIA) c) 18 (0) d) 1 (IA)
b) 17 (VIIA)
What is the total number of elements in Group 17 that are gases at room temperature and standard pressure? a) 1 b) 2 c) 3 d) 4
b) 2
Which group contains elements with a total of two electrons in the outermost principal energy level? a) 16 (VIA) b) 2 (IIA) c) 18 (0) d) 14 (IVA)
b) 2 (IIA)
Which sequence of atomic numbers represents elements which have similar chemical properties? a) 9,16,33,50 b) 4,20,38,88 c) 3,12,21,40 d) 19,23,30,36
b) 4,20,38,88
Which aqueous salt solution has a color? a) BaSO₄ (aq) b) CuSO₄ (aq) c) SrSO₄ (aq) d) MgSO₄ (aq)
b) CuSO₄ (aq)
Element X reacts with copper to form the compounds CuX and CuX₂. In which group on the periodic table is element X found? a) Group 13 b) Group 17 c) Group 1 d) Group 2
b) Group 17
The oxide of metal X has the formula XO. Which group in the periodic table contains metal X? a) Group 1 b) Group 2 c) Group 13 d) Group 17
b) Group 2
According to the reference table, which sequence correctly places the elements in order of increasing ionization energy? a) H→Li→Na→K b) I→Br→Cl→F c) O→S→Se→Te d) H→Be→Al→Ga
b) I→Br→Cl→F
Which element at room temperature is a poor conductor of electricity and has a relatively high electronegativity? a) Cu b) S c) Mg d) Fe
b) S
Which element is a liquid at room temperature? a) cesium b) bromine c) francium d) iodine
b) bromine
As the elements from Group 15 are considered from Group 15 are considered from top to bottom, the first ionization energy of the elements a) increases, and the electronegativity decreases b) decreases, and the electronegativity decreases c) increases, and the electronegativity increases d) decreases, and the electronegativity increases
b) decreases, and the electronegativity decreases
Compared to atoms of metals, atoms of nonmetals generally have a) higher electronegativities and lower ionization energies b) higher electronegativities and higher ionization energies c) lower electronegativities and higher ionization energies d) lower electronegativies and lower ionization energies
b) higher electronegativities and higher ionization energies
At which location in the periodic table would the most active metallic element be found? a) in Group 1 at the top b) in Group 1 at the bottom c) in Group 17 at the top d) in Group 17 at the bottom
b) in Group 1 at the bottom
As elements in a group of the periodic table are considered in order from top to bottom, the metallic character of each successive element generally a) decreases b) increases c) remains the same
b) increases
As the elements in Group 2 (IIA) are considered from beryllium to radium, the degree of metallic activity. a) decrease and atomic radius increases b) increases and atomic radius increases c) decreases and atomic radius decreases d) increases and atomic radius decreases
b) increases and atomic radius increases
Because of its high reactivity, which element is normally obtained by the electrolysis of its fused salts? a) sulfur b) lithium c) argon d) gold
b) lithium
Which group of elements occur only as compounds in nature because they are extremely reactive? a) 18 (0) b) (16) VIA c) 1 (IA) d) 11 (IB)
c) 1 (IA)
Which group contains elements composed of diatomic molecules at STP? a) 7 (VIIB) b) 17 (VIIA) c) 11 (IB) d) 2 (IIA)
c) 11 (IB)
In which group of elements do the atoms gain electrons most readily? a) 1 b) 2 c) 16 d) 18
c) 16
Which group on the period table has at least one element in each of the three phases of matter at STP? a) 1 b) 2 c) 17 d) 18
c) 17
Which element in Group 15 would most likely have luster and good electrical conductivity? a) N b) P c) Bi d) As
c) Bi
Which of the following aqueous solutions is blue? a) K₂SO₄ (aq) b) Na₂SO₄ (aq) c) CuSO₄ (aq) d) MgSO₄ (aq)
c) CuSO₄ (aq)
Which atom has the greatest tendency to gain electrons? a) I b) Rb c) F d) Al
c) F
In which set do the elements exhibit the most similar chemical properties? a) N, O, and F b) Hg, Br, and Rn c) Li, Na, and K d) Al, Si and P
c) Li, Na, and K
Which statement best compares the atomic radius of a potassium atom and the atomic radius of a calcium atom? a) The radius of the potassium atom is smaller because of its smaller nuclear charge. b) the radius of the potassium atom is smaller because of its larger nuclear charge. c) The radius of the potassium atom is larger because of its smaller nuclear charge. d) The radius of the potassium atom is larger because of its larger nuclear charge.
c) The radius of the potassium atom is larger because of its smaller nuclear charge.
In the modern periodic table, the elements are arranged according to a) atomic mass b) oxidation number c) atomic number d) mass number
c) atomic number
Which property decreases when the elements in Group 17 are considered in order of increasing atomic number? a) melting point b) atomic mass c) electronegativity d) atomic radius
c) electronegativity
In the ground state, an atom of each of the elements in Group 2 has a different a) number of valence electrons b) number of electrons in the first shell c) first ionization energy d) oxidation state
c) first ionization energy
The atoms of which element require the greatest amount of energy to remove an electron? a) krypton b) neon c) helium d) argon
c) helium
The amount of energy required to remove the most loosely bound electron from an atom in the gaseous phase is called a) potential energy b) electron affinity c) kinetic energy d) ionization energy
c) kinetic energy
Which of these metals loses electrons most readily? a) calcium b) magnesium c) potassium d) sodium
c) potassium
As the atoms of the elements in Group 1 of the periodic table are considered from top to bottom, the number of valence electrons in the atoms of each successive element a) decreases b) increases c) remains the same
c) remains the same
Compared to an atom of potassium, an atom of calcium has a a) larger radius and lower reactivity b) larger radius and higher reactivity c) smaller radius and lower reactivity
c) smaller radius and lower reactivity
Potassium forms an ion with a charge of a) 1- by gaining one electron b) 1- by losing one electron c) 1+ by gaining one electron d) 1+ by losing one electron
d) 1+ by losing one electron
Which value represents the first ionization energy of a nonmetal? a) 497.9 kJ b) 577.4 kJ c) 811.7 kJ d) 1000. kJ
d) 1000. kJ
A nonmetal could have an electronegatvity of a) 1.0 b) 2.0 c) 1.6 d) 2.6
d) 2.6
Which statement describes the elements in Period 3? a) Each successive element has a greater atomic radius b) Each successive element has a lower electronegativity c) All elements have similar chemical properties d) All elements have valence electrons in the same principal energy level
d) All elements have valence electrons in the same principal energy level
Atoms of which element have the smallest radius? a) Si b) P c) S d) Cl
d) Cl
Which element in Group 17 is the most active nonmetal? a) Br b) I c) Cl d) F
d) F
Which halogen can only be prepared from its fused compounds? a) 1₂ b) Cl₂ c) Br₂ d) F₂
d) F₂
Which of the following Group 15 elements has the most nonmetallic properties? a) Bi b) P c) Sb d) N
d) N
Which ion has the smallest radius? a) Te²- b) Se²- c) S²- d) O²-
d) O²-
Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? a) electronegativity increases, and ionization energy decreases b) electronegativity decreases, and ionization energy increases c) electronegativity and first ionization energy both decrease d) electonegativity and first ionization energy both increase
d) electonegativity and first ionization energy both increase
As the elements in Period 3 are considered from left to right, they tend to a) lose electrons more readily and increase in metallic character b) lose electrons more readily and increase in nonmetallic character c) gain electrons more readily and increase in metallic character d) gain electrons more readily and increase in nonmetallic character
d) gain electrons more readily and increase in nonmetallic character
Which properties are most common in nonmetals? a) low ionization energy and low electronegativity b) low ionization energy and high electronegativity c) high ionization energy and lower electronegativity d) high ionization energy and high electronegativity
d) high ionization energy and high electronegativity
Which element exhibits a crystalline structure at STP? a) fluorine b) bromine c) chlorine d) iodine
d) iodine
A reason why fluorine has a higher ionization energy than oxygen is that fluorine has a a) larger number of neutrons b) smaller nuclear charge c) smaller number of neutrons d) larger nuclear charge
d) larger nuclear charge
Which of the following metals has the lowest melting point? a) silver b) copper c) iron d) mercury
d) mercury
All the elements in Period 3 have the same number of a) electron b) protons c) occupied sublevels d) principal energy levels
d) principal energy levels
In which area of the periodic table are the elements with the strongest nonmetallic properties located? a) lower left b) upper left c) lower right d) upper right
d) upper right