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electron arrangement and periodic law
Terms in this set (49)
The Bohr model of the atom was an attempt to explain hydrogens
atomic emission spectrum
A bright-line spectrum (atomic emission spectra) of an atom is caused by the energy released when
fall to a lower energy level.
The lowest energy state of an atom is called the
What is the maximum number of orbitals in the d sublevel?
The major difference between a Is orbital and a 2s orbital is that
the 2s orbital is at a higher energy level.
How many unpaired electrons are there in a selenium atom (atomic number 34)?
Identify the element with the following electron configuration: ls^2s^2p^3s^3p^4s^3d"4p^
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be
distributed in the three orbitals?
one electron in each orbital
The group of soft, silvery active metals, all of which have 1 electron in an s orbital, is known as the
What is the chief characteristic of the noble gases?
very low reactivity.
Each period in the periodic table corresponds to
a principal energy level.
What is true of the electron configurations of the noble gasses
The outermost s and p sub levels are filled
What orbital is filled when iodine gains an electron to become a negative ion
valence electrons are those
in the highest energy level
How many valence electrons does an atom of any halogen have?
The number of valence electrons in Group 2 elements is
When an aluminum atom losesjts valence electrons, the charge on the resulting ion is
To attain a noble gas configuration a sulfur atom must
gain 2 electrons
How does atomic radius change from left to right across a period in the periodic table?
it tends to decrease
How does atomic radius change down a group in the periodic table?
it tends to increase
Heisenberg's uncertainty principle states that
it is impossible to know the position and velocity of an electron simultaneously
Greek philosopher who named the smallest particle of matter "atomos".
Believed that all atoms of an element were identical.
Discovered the electron/ Determined the charge on an electron.
The electron could circle the nucleus only in allowed paths, or orbits.
modeled orbitals as electron clouds with different shapes and sizes
Confirmed the existence of neutrons.
Region of high probability of finding an electron,
Tendency of electrons to enter orbitals of lowest energy first.
Arrangement of electrons around an atoms nucleus
Pauli Exclusion Principle
No more than two electrons can occupy an atomic orbital and these two electrons must have opposite spin.
when electrons occupy orbitals of equal energy, one electron enters each orbital until all orbitals contain one electron with parallel spins
ductile, form cations (positive), conductors
anions (negative), brittle, not conductive
metal and non metal characteristics, semi conductors
What principles or rules guide the electron configuration of an atom?
Aufbau principle, Pauli exclusion principle, Hunds rule
Describe Mendeleev's contribution to the periodic table. Why did he leave gaps in his table? What were the major
limitations of his periodic table?
first periodic table, gaps were left because not all elements were known, a limitation was it wasn't organized by atomic number
How does Moseley's periodic arrangement of the elements differ from Mendeleev's?
arranged by atomic number, not mass
the energy change that occurs when an electron is acquired by a neutral atom
A positive ion that formed from an atom losing an electron
the energy required to remove one electron from a neutral atom of an element
the tendency for the electrons in the inner energy levels to block the attraction of the nucleus for the valence electrons.
the strength of the nucleus to hold (attract) the outer electrons due to an increase of protons in the nucleus
A negative ion formed by the gain of electrons
Atomic radii generally "WHAT" as you move from left to right in a given period and WHY
decreases; because there is an increase in
the nuclear charge while the number of inner electrons, and hence the shielding effect, remains constant.
Atomic radii generally "WHAT" within a given group and WHY
increases; because the outer electrons are farther from the nucleus as you go
down the group. The attractive force ofthe increased nuclear charge is unable to overcome the effect ofthe greater
distance, which acts in opposition.
Ionization energy generally WHAT as you move from left to right across a period. Ionization energy, WHAT as you move down a group
Electronegativity generally WHAT as you move from left to right across a period. Electronegativity WHAT as you move down a group.
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