Periodic properties Flashcards
(25 cards)
A group of elements have the same amount of ___ ___
valence electrons
a period of elements have the same amount of ___ ___
electron shells
Transition metals show variable ____, can have multiple __ ___. they have this property because they have several electrons with similar __ __, meaning that one or all of them can be removed depending on the circumstances
valence, oxidation states, energy states
Most transition metals have ____ except row ____
colour, 4
The inner transition metals have their valence electrons in the inner __ orbital while transition metals have their valence electrons in their outer ___ orbitals. The most prominent oxidation state for transition metals is __, while for inner transition metals is ___. Inner transition metals are also far less ____.
f, d, 2+, 3+, abundant
atoms that exist in pair due to unstable nature
diatomic atoms
Metals are __, and ___, good conductors of __ and __, form ___ oxides, ___ electrons to form cations, __ at room temperature (except mercury) and have high __ and __ points
malleable, lustrous, heat, electricity, basic, lose, solid, boiling, melting
Non metals are __ and __, a poor conductors of electricity and heat, form __ oxides, gain electrons to form ___, are __ or ___ are room temperature (except bromine) and have ___ melting and boiling points
brittle, dull, acidic, anions, gas, solid, low
1/2 the distance between the nuclei of two identical atoms bonded together
atomic radius
atomic radius decreases ___ to ___ due to more ______ exerting a greater nuclear attraction between protons and electrons. They also get larger going __ a group, because there are more electrons, and the addition of a new __ ___< and each new shell gets further away from the nucleus
left, right, protons, down, electron shell
The amount of positive charge experienced by an electron
effective nuclear charge
The __ ___ of lower orbital electrons prevents higher orbital electrons from experiencing a __ ___ to the nucleus. This explains the easy removal of ___ ____.
shielding effect, strong attraction, valence electrons
Equation for Zeff
Zeff = Z (# of protons) - S (# of shielding electrons / non valence electrons)
The Zeff ____ from left to right due to the increase in the number of ____. Zeff ___ going up a group.
increases, protons, increases
atoms with identical number of electrons and differing number of protons
isoelectronic series
The energy needed to remove an electron from an atom
ionization energy
ionization energy increases from left to right, due to the number of __ and ___ increasing. As the __ ___ fills, the electrons become harder to remove. As you go up a group the ionization energy also increases because there are less __ ___, and thus the electrons are closer to the nucleus
electrons, protons, valence electrons, energy levels
Following removal of the 1st electron, elements can have subsequent ionization energies whose values are __ ___.
always higher
__ ___ ___ have greater ionization energy than group 13 elements. This is because they have __ ___, and thus it requires more energy to remove an electron. Also, group ___ have greater ionization than group ____ elements. This is because they have __ ___ orbitals and thus greater stability.
alkali earth metals, filled orbitals, 15, 16, half filled
the amount of energy released when an electron is added to an atom
electron affinity
Electron affinity increases from left to right, because the ___ of the valence shell results in a greater propensity to gain an electron. electron affinity increases as you move up a group due to more ___ between the nucleus and the electron, and a decreasing in the ____ effect that is in the way of the the new electrons
filling, attraction, shielding
Exceptions to the electron affinity are when elements obtain a ___ ____ ____ by gaining an electron, which gives it a greater affinity. ___ ____ have complete valence shells and thus have negligible electron affinities
stable half-filled subshell, noble gasses
the ability of an atom to attract electrons in a bond
electronegativity
electronegativity increases from left to right because of the increase in _____, which gives it its increased ability to attract electron ___ in a ___. Electronegativity increases up a group due to a decrease in __ __, which means the valence electrons experience less ___. __ ____ no electronegativity. ___ is the most electronegative atom
protons, pairs, bond, atomic radius, shielding, noble gases, F
