Chemistry I: Chapter 6
How many columns of elements does the periodic table contain?
18
How many rows of elements does the periodic table contain?
7
Which correctly describes elements in the same group? A. They have the same number of valence electrons B. They have electrons in the same outermost energy level C. They have the same atomic radius D. They must be in the same state of matter
A. They have the same number of valence electrons
An atom becomes negative charged by A. gaining an electron B. gaining a proton C. losing an electron D. losing a neutron
A. gaining an electron
What is the trend in atomic radii as you move from left-to-right across a period? A. generally decreases B. generally increases C. remains the same D. varies randomly
A. generally decreases
Which is defined as the energy required to remove an electron from an atom of an element in the gaseous state? A. ionization energy B. electronegativity C. ionic radius D. law of octets
A. ionization energy
Which energy level of the period 4 transition elements is being filled with electrons? A. third B. fourth C. fifth D. sixth
A. third
How many electrons does an atom generally need in its outer level to be the most stable? A. 4 B. 8 C. 10 D. 12
B. 8
Which metalloid is in the fourth period and the same group as Carbon? A. Silicon B. Germanium C. Tin D. Boron
B. Germanium
A(n) _____ is an atom, or bonded group of atoms, that has a positive or negative charge. A. halogen B. ion C. isotope D. molecule
B. ion
Which category of elements is commonly used to make computer chips and solar cells due to their ability to conduct electricity only under certain conditions? A. metals B. metalloids C. nonmetals D. noble gases
B. metalloids
Which category of elements have the property of being malleable and ductile? A. gases B. metals C. metalloids D. nonmetals
B. metals
Which block of element Y most likely found if: - Element X: s block; soft, shiny grey metal, highly reactive, lightweight - Element Y: ?; liquid at room temperature, has the highest electronegativity in its period - Element Z: p block; used as a semiconductor due to its electricity-conducting properties A. s B. p C. d D. f
B. p
Which of the following pair is the second particle listed larger than the first? A. K, Ga B. Pb, C C. Br, Br- D. Li, Li+
C. Br, Br-
Which is the halogen that is in Period 5? A. Bromine (Br) B. Strontium (Sr) C. Iodine (I) D. Xenon (Xe)
C. Iodine (I)
Which of the following elements is a metal? A. Boron B. Nitrogen C. Magnesium D. Carbon
C. Magnesium
Identify the period and group numbers of the element with the electron configuration [Ne] 3s2 3p4 A. Period 2, Group 4 B. Period 3, Group 4 C. Period 3, Group 16 D. Period 2, Group 16
C. Period 3, Group 16
Based on the information below, which element has the greatest number of valence electrons? Hydrogen: 1s1 Lithium: 1s2 2s1 Sodium: 1s2 2s2 2p6 3s1 Potassium: 1s2 2s2 2p6 3s2 3p6 4s1 A. lithium B. potassium C. They all have the same number of valence electrons D. The table does not show numbers of valence electrons
C. They all have the same number of valence electrons
Which block contains 5 orbitals? A. s B. p C. d D. f
C. d
Most of the elements in group 16 through 18 are classified as A. alkali metals B. inner transition metals C. nonmetals D. alkaline earth metals
C. nonmetals
Atomic radii cannot be measured directly because the electron cloud surrounding the nucleus does not have a clearly defined A. charge B. mass C. outer edge D. probablility
C. outer edge
Which is the most important characteristic in determining an element's chemical properties? A. the number of protons and neutrons in its nucleus B. which period it is found in C. the number of valence electrons it contains D. its outermost energy level
C. the number of valence electrons it contains
Which of the following classifications describes the element with the electron configuration [Ar] 4s2 3d10 4p5 A. stable metal B. stable nonmetal C. unstable nonmetal D. unstable metal
C. unstable nonmetal
In which pair is the one on the left larger than the one on the right? A. Na, Rb B. S, Mg C. Br, Br- D. K, K+
D. K, K+
Which scientist first arranged elements by atomic number? A. Mendeleev B. Lavoisier C. Newlands D. Mosely
D. Mosely
What do the elements of a group (family) have in common? A. They have the same atomic number B. They have the same atomic mass C. They have the same number of protons D. They have the same number of valence electrons
D. They have the same number of valence electrons
Which of the following electron configurations represents the most chemically stable atom? A. [He] 2s2 2p3 B. [Ne] 3s2 3p5 C. [Ne] 3s2 4s2 3d5 D. [Ne] 3s2 3p6
D. [Ne] 3s2 3p6
Which block on the periodic table contains the actinide series of elements? A. s-block B. p-block C. d-block D. f-block
D. f-block
Elements in the same group have the same A. atomic radius B. energy level of outer electrons C. nuclear charge D. number of valence electrons
D. number of valence electrons
Identify the period and group of the element that has the electron configuration of [Ne] 3s2 3p3 A. period 2, group 2 B. period 3, group 1 C. period 3, group 13 D. period 3, group 15
D. period 3, group 15
The trend in the atomic radii as you move down the group 1 elements is partially due to A. decreased distance of outer electrons B. increased nuclear charge C. increased number of electrons in outer energy level D. shielding by inner electrons
D. shielding by inner electrons
The general trend in the radius of an atom moving down a group is partially accounted for by the A. decrease in mass of the nucleus B. fewer number of filled orbitals C. increase in the charge of the nucleus D. shielding of the outer electrons by inner electrons
D. shielding of the outer electrons by inner electrons
The first periodic table is mostly credited to _____ _____.
Dmitri Mendeleev
What can be said about the electron configurations of all the elements in a group?
They have the same number of valence electrons
The law of octaves did not work for all known elements was not generally _____.
accepted
Group 1 elements (except for hydrogen)
alkali metals
What is the name of the group 1 elements (excluding hydrogen)?
alkali metals
Group 2 elements
alkaline earth metals
What is the name of the group 2 elements?
alkaline earth metals
where are the metalloids located
along stairstep (except aluminum)
In Mendeleev's table, the elements were arranged according to increasing _____ _____.
atomic mass
The element in the periodic table are arranged to increasing _____ _____, as the result of of the work of _____ _____.
atomic number Henry Mosely
What is the trend for atomic radii?
bigger going down, bigger going left
what block are the transition metals located
d block
According to the law of octaves, the properties of the elements repeated every _____ elements.
eight
indication of an atom's ability to attract electrons in a chemical bond
electronegativity
One important result of Mendeleev's table was that the existence and properties of undiscovered _____ could be predicted
elements
What is ionization energy?
energy required to remove an electron from an atom
what block are the inner transition metals located
f block
True or False: All the nonmetals on the periodic table are gases
false
True or False: An atom that gains an electron will form a positive ion
false
True or False: Elements in Group 2 are classified as alkali metals
false
True or False: Group 13 elements are the alkaline earth metals
false
True or False: Group 18 elements are very unreactive elements known as transition metals
false
True or False: Metalloids have properties of both metals and inner transition metals
false
True or False: More than 3/4 of the elements in the periodic table are nonmetals
false
True or False: The electronegativity of elements increase from left to right and from top to bottom on the periodic table
false
True or False: The same amount of energy is required to remove each election sequentially from an atom
false
True or False: There are two main classifications of elements
false
What is the trend of electronegativity?
gets bigger going up, gets bigger going right
A column in the periodic table
group
What is another name for a column of elements?
group/family
Group 17 elements
halogens
What is the name of the group 17 elements?
halogens
What is the trend for ionization energy?
increases going up, increases going right
Atom or bonded group of atoms that has a positive or negative charge
ion
energy required to remove an electron from a gaseous atom
ionization energy
Explain why an atom with high ionization energy value is most not likely to form a positive ion
it needs a lot of energy to remove an electron, so it's not likely
Is most the periodic table metals or nonmetals?
metals
According to the law of octaves element two and _____ have similar properties.
nine
Group 18 elements
noble gases
What is the name of group 18 elements?
noble gases
John Newlands developed the law of _____.
octaves
statement that atoms tend to gain, lose, or share electrons to acquire a full set of eight valence electrons
octet rule
A row in the periodic table
period
What is another name for a row of elements?
period
Statement that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties
periodic law
The modern form of the periodic table result in the _____ _____, which states that when elements are arranged according to increasing atomic number there is a periodic repetition of their chemical and physical _____.
periodic law properties
The arrangement of the modern periodic table is based on number of _____ in the nucleus of an atom of the element.
protons
Groups 1 and 2, 13 through 18
representative elements
Groups 3 through 12
transition elements
True or False: Elements in Group 17 are classified as halogens
true
True or False: Elements in the same family tend to have the same number of valence electrons
true
True or False: Group 1 elements (except for hydrogen) are known as the alkali metals
true
True or False: Group 17 elements are highly reactive nonmetals known as halogens
true
True or False: The octet rule states that atoms will gain, lose, or share electrons to achieve the same number of valence electrons
true
True or False: When an atom loses electrons, its radius gets smaller
true