• Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off

Card Range To Study



Play button


Play button




Click to flip

Use LEFT and RIGHT arrow keys to navigate between flashcards;

Use UP and DOWN arrow keys to flip the card;

H to show hint;

A reads text to speech;

22 Cards in this Set

  • Front
  • Back
The periodic law states that the properties of elements are periodic functions of their atomic numbers. What determines the position of each element in the periodic table?
a. mass number
b. number of protons
c. number of neutrons
d. number of isotopes
When determining the size of an atom by measuring the distance between bonded, identical, adjacent nuclei, the radius of an atom is
a. equal to the distance between nuclei.
b. one-half the distance between nuclei.
c. one-fourth the distance between nuclei.
d. twice the distance between nuclei.
The discovery of what elements added a new column to Mendeleev's periodic table?
a. radioactive elements
b. metalloids
c. noble gases
d. transition elements
In Period 3 there are 8 elements. What sublevel(s) is (are) being filled?
a. s and d
b. d and f
c. s and p
d. s
The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
a. Ramsey.
b. Mendeleev.
c. Bohr.
d. Moseley.
When an electron is aquired by a neutral atom, the energy change is called
a. ionization energy.
b. electron configuration.
c. electronegativity.
d. electron affinity.
Compared to the alkali metals, the alkaline-earth metals
a. combine more readily with nonmetals.
b. have lower melting points.
c. are less reactive.
d. are less dense.
The energy required to remove an electron from an atom is the atom's
a. electronegativity.
b. ionization energy.
c. electron affinity.
d. electron energy.
A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called
a. electron configuration
b. electron affinity
c. electronegativity
d. ionization potential.
The number of valence electrons in Group 17 element is
a. 17.
b. 8.
c. 7.
d. equal to the period number.
Elements in a group or column in the periodic table can be expected to have similar
a. numbers of neutrons.
b. properties.
c. atomic masses.
d. atomic numbers.
The electrons available to be lost, gained, or shared when atoms form compounds are called
a. valence electrons
b. d electrons
c. ions.
d. electron clouds.
Elements in which the d-sublevel is being filled have the properties of
a. nonmetals.
b. metalloids.
c. metals.
d. gases.
Which block in the periodic table contains the alkali metals?
a. s
b. p
c. f
d. d
For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number
a. plus 5.
b. minus 10.
c. plus 1.
d. minus 1.
A horizontal row of blocks in the periodic table is called a(n)
a. group.
b. family.
c. octet.
d. period.
The person whose work led to the periodic table based on increasing atomic number was
a. Cannizzaro.
b. Mendeleev.
c. Rutherford.
d. Moseley.
In a row in the periodic table, as the atomic number increases, the atomic radius generally
a. remains constant.
b. decreases.
c. increases.
d. becomes immeasurable.
The periodic table
a. was completed with the dicovery of the noble gases.
b. will be completed with element 118.
c. has been of little use to chemists since the early 1900s.
d. permits the properties of an element to be predicted before the element is discovered.
As you move down Group 14 in the periodic table from carbon through lead, atomic radii
a. vary unpredictably.
b. generally decrease.
c. generally increase.
d. do not change.
Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a. A new octet forms.
b. The number of neutrons increases.
c. The number of occupied energy levels increases.
d. The nuclear charge increases.
How does electronegativity change as we move across a period? Explain why this occurs.
Electronegativity generally increases as we move across a period. This occurs because the trend is going lowest to highest from the bottom left corner to the upper right. This occurs because the number of protons in the nucleus goes up and the more protons there are the more they are attracting electrons.