Periodic properties

Question 1

A group of elements have the same amount of ___ ___

Answer 1

valence electrons

Question 2

a period of elements have the same amount of ___ ___

Answer 2

electron shells

Question 3

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

Answer 3

valence, oxidation states, energy states

Question 4

Most transition metals have ____ except row ____

Answer 4

colour, 4

Question 5

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 ____.

Answer 5

f, d, 2+, 3+, abundant

Question 6

atoms that exist in pair due to unstable nature

Answer 6

diatomic atoms

Question 7

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

Answer 7

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

Question 8

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

Answer 8

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

Question 9

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

Answer 9

atomic radius

Question 10

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

Answer 10

left, right, protons, down, electron shell

Question 11

The amount of positive charge experienced by an electron

Answer 11

effective nuclear charge

Question 12

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

Answer 12

shielding effect, strong attraction, valence electrons

Question 13

Equation for Zeff

Answer 13

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

Question 14

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

Answer 14

increases, protons, increases

Question 15

atoms with identical number of electrons and differing number of protons

Answer 15

isoelectronic series

Question 16

The energy needed to remove an electron from an atom

Answer 16

ionization energy

Question 17

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

Answer 17

electrons, protons, valence electrons, energy levels

Question 18

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

Answer 18

always higher

Question 19

__ ___ ___ 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.

Answer 19

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

Question 20

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

Answer 20

electron affinity

Question 21

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

Answer 21

filling, attraction, shielding

Question 22

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

Answer 22

stable half-filled subshell, noble gasses

Question 23

the ability of an atom to attract electrons in a bond

Answer 23

electronegativity

Question 24

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

Answer 24

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

Question 25

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

Answer 25

down, left, up, right