Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar ___.

Mendeleev predicted that the spaces in his periodic table represented ___.

The periodic table ___.

Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing ___.

What are the elements whose discovery added an entirely new column to Mendeleev's periodic table?

John Newlands called his ideas about the arrangement of the elements ___.

Dobereiner's method of calculating physical properties ___.

In 1869, the number of known elements was ___.

The work that lead to use of atomic numbers ___.

The most abundant element of the surface of Earth is ___.

The element that appears with the Group 1A elements but is not a metal is ___.

The length of each period in the periodic table is determined by the ___.

When an electron is added to an atom or ion, the radius ___.

As you move left to right from gallium through bromine, atomic radii ___.

A positive ion is known as a(n) ___.

The most characteristic property of the noble gasses is that they ___.

In nature, the alkali metals occur as ___.

Two Group VA elements essential to life are ___.

The alkali metals belong to the ____-block in the periodic table.

Hydrogen is placed separately from other elements in the periodic table because it ___.

For each successive electron removed from an atom, the ionization energy ___.

The element that has the greatest electronegativity is ___.

A measure of the ability of an atom in a chemical compound to attract electrons is called ___.

In a row in the periodic table, as the atomic number increases, the atomic radius generally ___.

Among the d-block elements, as atomic radii decrease, electronegativity values ___.

The energy required to remove an electron from an atom is the atom's ___.

The elements that border the zigzag line in the periodic table are ___.

Valence electrons are those ___.

In addition to graphite and diamond, elemental carbon has other allotropes recently discovered known as ___.

Nitrogen in the atmosphere is incorporated into amino acids in the biosphere by ___.

In addition to oxygen, silicon, and aluminum, the most abundant elements that make up the rocks in the Earth's crust include ___.

Dissolved phosphate acids and salts are used in animal metabolism ___.

The period of an element can be determined from its ___.

The unique ability of carbon atoms to form long chains, apparently necessary to biology, is known as ___. (INCORRECT)

Neutral atoms with an s2p6 electron configuration in the highest energy level are best classified as ___.

To which group do lithium and potassium belong?

Long term sources of heat energy input to the Earth include solar radiation and ___.

Boron is said to be electron deficient, which ___.

If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is ___.

The lanthanides series of elements are known as the Rare Earth metals.  Except for promethium, all are more abundant naturally in the Earth's crust than ___.

The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period ___.

Oxygen makes up about ___ of the Earth's crust.

The group of 14 elements in the sixth period that have occupied 4f orbitals is the ___.

To which group do fluorine and chlorine belong?

Elements in which the d-sublevel is being filled have the properties of ___.

Current uses of hydrogen H2 include all the following EXCEPT ___.

The only metal in the fifth period known to be essential to life is ___.

The elemental form that halogens adopt is ___.

After fluorine, the most electronegative element is ___.

Two transition metal elements essential to life are ___.

Phosphorus is a constituent part of ___.

Ionization energy is the energy required to remove ___ from an atom of an element.

Magnesium has the electron configuration [Ne] 3s2. To what group does magnesium belong?

Elements to the right side of the periodic table (p-block elements) have properties most associated with ___.

Titanium, atomic number 22, has the configuration [Ar] 3d2 4s2. To what group does titanium belong?

In the periodic table, the periods are the ___.

The most abundant element in the universe is ___.

In the alkaline-earth group, atoms with the smallest radii ___.

White phosphorus ___.

Elements on the right side of the periodic table (p-block elements) have properties most associated with ___.

In 1863 when evaluating the ideas of ___, all the experts were wrong.

How many elements are in the first period of the periodic table?

Nitrogen's electron configuration is 1s2 2s2 2p3. To what group does nitrogen belong?

Dalton compared the masses of the elements known at his time to the mass of ___.

Elements in a group or column in the periodic table can be expected to have similar ___.

An example of a lanthanide element is ___.

The elements with electron configurations ending with s2 p5 in the highest occupied energy level belong to Group ___.

The alkali metals belong to the ___-block in the periodic table.

The valence electrons in an atom are always ___.

An example of an actinide element is ___.

Which of the following is represented by the abbreviated electron configuration of an atom of an element?

The person whose work led to a periodic table based on increasing atomic number was ___.

When an electron is added to a neutral atom, a certain amount of energy is ___.

The force of attraction by Group 1 metals for their valence electrons is ___.

The electrons available to be lost, gained, or shared when atoms form molecules are called ___.

Within a group of elements, as the atomic number increases, the atomic radius ___.

When an electron is removed from an atom or ion, the radius ___.

Which block of the periodic table contains both metals and nonmetals?

The electron configurations of the noble gases from neon to radon in the periodic table end with filled ___.

The most reactive group of the nonmetals are the___.