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Chemistry - Ch. 6 Test
ability of an atom to attract electrons when the atom is a compound
type of ion formed by group 2A elements
type of element characterized by the presence of electrons in the d orbital
vertical column in the periodic table
subatomic particles that are transferred to form positive and negative ions
horizontal row in the periodic table
one-half the distance between the nuclei of two atoms when the atoms are joined
energy required to remove an electron from an atom
a repetition of properties occurs when elements are arranged in order of increasing atomic number
type of element that is a good conductor of heat and electric current
decreases with increasing atomic number in group 2A
groups 3A through 8A
elements characterized by filling of p orbitals
subatomic particle that plays the greatest part in determining the properties of an element
electrons are added to the same principle energy level
what causes the shielding effect to remain constant across a period?
group A elements
another name of the representative elements
an increase in the number of protons
what contributes to the increase in ionization energy from left to right across a period>
element with the highest electronegativity value
for group 2A metals which electron is the most difficult to remove?
decreases as you move from left to right across a period
atomic size generally
cations form when an atom loses electrons.
what is true about ions?
what is the element with the lowest electronegativity value?
a filled highest occupied principle energy level
what electron configuration is most likely to result in an element that is relatively inactive?
what element in the second period has the largest atomic radius?
it tends to decrease
how does atomic radius change from left to right across a period in the periodic table?
it tends to increase
how does atomic radius change from top to bottom in a group in the periodic table?
a principle energy level
each period in the periodic table corresponds to
group B elements
another name for transition metals
the modern periodic table is arranged in order of increasing atomic
electronegativity generally increases from left to right across a period.
what is true about electronegativity?
poor conductors of electricity
who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
which of the following elements has the smallest first ionization energy? sodium, magnesium, calcium, potassium
which of the following elements has the smallest ionic radius? S, Li, O, K
group in the periodic table whose elements have the highest electronegativity values
group 1A elements
alkaline earth metals
group 2A elements
ions formed from elements in group 7A
group 7A elements (nonmetals)
decreases for cations and anions from left to right across a period\
inner transition metals
highest occupied s sublevels and a nearby f sublevel contain electrons