Chemistry - Ch. 6 Test

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electronegativity

ability of an atom to attract electrons when the atom is a compound

cation

type of ion formed by group 2A elements

transition metal

type of element characterized by the presence of electrons in the d orbital

group

vertical column in the periodic table

electrons

subatomic particles that are transferred to form positive and negative ions

period

horizontal row in the periodic table

atomic radius

one-half the distance between the nuclei of two atoms when the atoms are joined

ionization energy

energy required to remove an electron from an atom

periodic law

a repetition of properties occurs when elements are arranged in order of increasing atomic number

metal

type of element that is a good conductor of heat and electric current

ionization energy

decreases with increasing atomic number in group 2A

groups 3A through 8A

elements characterized by filling of p orbitals

electron

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>

fluorine

element with the highest electronegativity value

the third

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?

cesium

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?

lithium

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

number

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

nonmetals are

mendeleev

who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?

potassium

which of the following elements has the smallest first ionization energy? sodium, magnesium, calcium, potassium

Li

which of the following elements has the smallest ionic radius? S, Li, O, K

halide ions

group in the periodic table whose elements have the highest electronegativity values

alkali metals

group 1A elements

alkaline earth metals

group 2A elements

halide ions

ions formed from elements in group 7A

halogens

group 7A elements (nonmetals)

ionic radius

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

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