Periodic properties Flashcards

1
Q

A group of elements have the same amount of ___ ___

A

valence electrons

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2
Q

a period of elements have the same amount of ___ ___

A

electron shells

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3
Q

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

A

valence, oxidation states, energy states

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4
Q

Most transition metals have ____ except row ____

A

colour, 4

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5
Q

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 ____.

A

f, d, 2+, 3+, abundant

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6
Q

atoms that exist in pair due to unstable nature

A

diatomic atoms

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7
Q

Metals are __, and ___, good conductors of __ and __, form ___ oxides, ___ electrons to form cations, __ at room temperature (except mercury) and have high __ and __ points

A

malleable, lustrous, heat, electricity, basic, lose, solid, boiling, melting

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8
Q

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

A

brittle, dull, acidic, anions, gas, solid, low

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9
Q

1/2 the distance between the nuclei of two identical atoms bonded together

A

atomic radius

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10
Q

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

A

left, right, protons, down, electron shell

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11
Q

The amount of positive charge experienced by an electron

A

effective nuclear charge

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12
Q

The __ ___ of lower orbital electrons prevents higher orbital electrons from experiencing a __ ___ to the nucleus. This explains the easy removal of ___ ____.

A

shielding effect, strong attraction, valence electrons

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13
Q

Equation for Zeff

A

Zeff = Z (# of protons) - S (# of shielding electrons / non valence electrons)

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14
Q

The Zeff ____ from left to right due to the increase in the number of ____. Zeff ___ going up a group.

A

increases, protons, increases

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15
Q

atoms with identical number of electrons and differing number of protons

A

isoelectronic series

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16
Q

The energy needed to remove an electron from an atom

A

ionization energy

17
Q

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

A

electrons, protons, valence electrons, energy levels

18
Q

Following removal of the 1st electron, elements can have subsequent ionization energies whose values are __ ___.

A

always higher

19
Q

__ ___ ___ 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.

A

alkali earth metals, filled orbitals, 15, 16, half filled

20
Q

the amount of energy released when an electron is added to an atom

A

electron affinity

21
Q

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

A

filling, attraction, shielding

22
Q

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

A

stable half-filled subshell, noble gasses

23
Q

the ability of an atom to attract electrons in a bond

A

electronegativity

24
Q

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

A

protons, pairs, bond, atomic radius, shielding, noble gases, F

25
Q

metallic character increases as you move ____ and to the ______. Non metallic character increases as you move ______ and to the ___

A

down, left, up, right