Ch 6: The Periodic Table Flashcards
Chemists use the __________ of elements to sort them into ______.
properties
groups
Who published a classification system in which he grouped elements into triads?
J. W. Dobereiner
Who arranged the elements in his periodic table in order of increasing atomic mass?
Mendeleev
How are elements arranged in the modern periodic table?
In order of increasing atomic number.
What are the three classes of elements?
- Metals
- Nonmetals
- Metalloids
The periodic table displays the _______ and _____ of the elements along with information about the _________ of their atoms.
symbols
names
structure
Elements can be sorted into _____ _____, ______________ ________, __________ ______, or _____ __________ ______ based on their electron configuration.
noble gases
representative elements
transition metals
inner transition metals
What is the distance from the nucleus to the furthermost electron referred to as?
Atomic radius
In general, atomic size _________ from top to bottom within a group and _________ from left to right across a period.
increases
decreases
Atomic radius: largest value
Bottom left
Atomic radius: smallest value
Top right
Atomic radius: group trends
The amount of energy levels is increasing.
Atomic radius: periodic trends
Gaining protons.
Positive and negative ions form when _________ are transferred between atoms.
electrons
What is the amount of energy needed to remove the most loosely held electron referred to as?
Ionization energy
Ionization energy tends to ________ from top to bottom within a group and ________ from left to right across a period.
decrease
increase
Ionization energy: largest value
Top right
Ionization energy: smallest value
Bottom left
Ionization energy: group trends
Farther from the nucleus, electron is easier to lose.
Ionization energy: periodic trends
The atoms are getting smaller/closer to the nucleus.
Cations are always _______ than the atoms from which they form. Anions are always ______ than the atoms from which they form.
smaller
larger
Metals form positively charged ions by ______ electrons.
Losing
Cations: groups
Increase ionic radius
Cations: periods
Decrease ionic radius
Nonmetals form negatively charged ions by _______ electrons.
Gaining
Anions: groups
Decrease ionic radius
Anions: periods
Increase then decrease ionic radius
What is the relative attractiveness an atom has for its shared electrons?
Electronegativity
Electronegativity values ________ from top to bottom with a group.
Decrease
Why does electronegativity decrease from top to bottom?
Farther from the nucleus.
For representative elements, the values tend to ________ from left to right across a period.
Increase
Why does representative element values increase from left to right?
Closer to the nucleus.
Representative elements: largest value
Top right
Representative elements: smallest value
Bottom left
The trends that exist among these properties can be explained by variations in ______ _________.
atomic structure
