Orbitals, Electrons, Periodic Trends, And Bonding

Front 1

high energy electrons are where with respect to the atomic nucleus?

Back 1

further from the Atomic nucleus = higher energy

Front 2

A period of the periodic table is the _____

Back 2

Columns (up-down on table) of elements to represent
1s
2s
2p
3s
3p
....
Elements of the same period have the same number of electron shells; with each group across a period, the elements have one more proton and electron and become less metallic.

Front 3

a group in the periodic table is the _____

Back 3

rows (left to right). They share similar electron numbers in their outer shell

The elements in a group have similar physical or chemical characteristic of the outermost electron shells of their atoms (i.e., the same core charge), as most chemical properties are dominated by the orbital location of the outermost electron.

Front 4

Characteristics of metallic elements and the reason for metallic bonds

Back 4

Atoms of metals readily lose their outer shell electrons, resulting in a free flowing cloud of electrons within their otherwise solid arrangement. This provides the ability of metallic substances to easily transmit heat and electricity. While this flow of electrons occurs, the solid characteristic of the metal is produced by electrostatic interactions between each atom and the electron cloud

The lower the values of ionization energy, electronegativity and electron affinity, the more metallic character the element has

Front 5

atomic number represents?

Back 5

the number of protons in its nucleus

Front 6

atomic weight

Back 6

protons and neutrons

Front 7

what is the electron configuration of Silicon? Iodine? Chlorine? Potassium?

Back 7

Silicon - 1s2 2s2 2p6 3s2 3p2
Iodine - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
Potassium - 1s2 2s2 2p6 3s2 3p6 4s1
etc

Front 8

Where is there more metallic character? Higher atomic radius? Ionization energy? Electron affinity?

Back 8

Front 9

what is ionization energy?

Back 9

The first ionization energy is the energy it takes to remove one electron from an atom, the second ionization energy is the energy it takes to remove a second electron from the atom, and so on. Electrons in the closer orbitals experience greater forces of electrostatic attraction; thus, their removal requires increasingly more energy. Ionization energy becomes greater up and to the right of the periodic table

Front 10

what is electronegativity?

Back 10

In easy terms, the desire for the atom to steal an electron. Electronegativity is the tendency of an atom to attract electrons. An atom's electronegativity is affected by both its atomic number and the distance between the valence electrons and the nucleus.

In a covalent bond, the atom that is more electronegative will hog the electron more than the atom that is less electronegative.

Front 11

Electron affinity

Back 11

The electron affinity of an atom is the amount of energy released when an electron is added to a neutral atom to form a negative ion. Although electron affinity varies greatly, some patterns emerge. Generally, nonmetals have more positive electron affinity values than metals. Fluorine most strongly attracts an extra electron.

Front 12

Ions are? Cations and Anions?

Back 12

atoms with different number of electrons compared to protons. they can have more or less and are denoted by their ionic number

Cations are positive, hence t = +
Anions are negative, hence n = negative
Al3+, Cl−

Front 13

The ionization energy is?

Back 13

of an atom or molecule describes the minimum amount of energy required to remove an electron (to infinity) from the atom or molecule

Front 14

First column in periodic table is?

Back 14

Alkali metals, know SODIUM and POTASSIUM
lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr)

readily lose their outermost electron to form cations with charge +1.

Front 15

second column of periodic table?

Back 15

Alkali earth metals, know CALCIUM and MAGNESIUM
beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra)

readily lose their two outermost electrons to form cations with charge 2+ and an oxidation state, or oxidation number of +2.

Front 16

last column in periodic table?

Back 16

Noble gases
very LOW chemical reactivity. know HELIUM and NEON
The six noble gases that occur naturally are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and the radioactive radon (Rn).

Front 17

second to last column in periodic table?

Back 17

Halogens, FLUORINE, CHLORINE, IODINE
fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
This HIGH REACTIVITY is due to the high electronegativity of the atoms due to their high effective nuclear charge. They can gain an electron by reacting with atoms of other elements.

Front 18

How many electrons can be held in a shell?

Back 18

4ℓ + 2

4(1)+2= 6
etc etc

Front 19

shielding effect describes ?

Back 19

the attraction between an electron and the nucleus in any atom with more than one electron shell.

Front 20

What is unique about D block electron configurations in comparison to S and P block?

Back 20

The D block backfills a shell configuration, so if you already have 3p6 4s2, then you have 3d next.

The outermost energy shell is still the 4s2 because the D block is backfilling the previous shell. However, the D block are still the highest energy state electrons if they are the final ones in the electron configuration.

Front 21

What does the metallic nature of an element mean?

Back 21

It means it wants to give away electrons. they have a low ionization energy

Front 22

what is 2nd ionization energy?

Back 22

the energy required to remove the second electron

elements like Lithium (alkali metals) that have only one valence electron have a very high 2nd ionization energy

Front 23

what is somewhat counterintuitive about the size of an element in reference to its electron radius and placement on the periodic table?

Back 23

although the element is generally larger the lower you get on the periodic table as it contains more protons, neutrons, and electrons, the electrons actually get pulled closer to the nucleus the further filled the electron valence shells are and further right the element is on the periodic table.

Front 24

Covalent Bond

Back 24

Strongest bond, an atom which wants to give an electron bonds with an atom that wants to take an electron. Electron is shared.

The atom that is more electronegative will hog the electron more than the atom that is less electronegative.

ie O2, Oxygen has 6 valence electrons and two of the electrons are shared among the space between them so the atoms can pretend like they each have 8 (double bond)

More common with atoms that are similarly electronegative or the same element altogether, as in O2

Front 25

Ionic Bond

Back 25

An atom which wants to give an electron gives its electron to an atom that wants to take an electron. The donor atom is now positively charged, having more protons than electrons, and the receiver atom is now negatively charged. The charge of the two atoms draws them together.

ie NaCl, Na becomes a cation and Cl becomes an anion.

Front 26

Diatomic Molecules

Back 26

Molecule consisting of only 2 atoms, considered homonuclear if both the atoms are the same element and generally share as a covalent bond.

Picture of atoms that commonly present as homonuclear

Front 27

Polar Covalent Bond

Back 27

A covalent bond where, as in H2O, there is an atom that is more electronegative which causes a slight imbalance in charges on the atoms. In H2O, Oxygen is more electronegative and hogs Hydrogen's electrons, leaving Oxygen with a slightly negative charge. The two hydrogens are then slightly positive.

Front 28

Metallic Bond

Back 28

Several atoms who like to give up their electrons all share electrons in a communal electron area.

i.e. 4 Fe atoms together will become more positively charged as they give off electrons to be in this shared zone

Makes these elements more conductive to electricity because their electrons can move around much easier, also makes element more malleable.