Science UNIT 2.1-2.2 Test Flashcards

2.1: Atoms and electronic configuration, 2.2: Trends in the Periodic Table

1s2, 2s2, 2p6 ,3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10, 5p6, 6s2, 4f14, 5d10, 6p6, 7s2, 5f14, 6d10, 7p6

Recite the Moeller Diagram.

Boron, Silicon, Germanium, Astatine, Antimony, Polonium, Tellurium, Arsenic.

Name all the metalloids in the periodic table. (8)

The metals of the periodic table are mostly found on the left and center of the periodic table.

A zigzag staircase line separates them from the metalloids and non-metals.

The center of the periodic table, mostly the d-block, contains all the transition metals, which are mostly metallic.

The left side of the periodic table (groups 1 and 2), which contains the alkali metals and alkali earth metals, are entirely metallic.

Where are the metals of the periodic table found?

The non-metals of the periodic table are primarily found on the right side of the table. A zigzag staircase line, starting from boron, separates the non-metals from the metals.

Hydrogen, although being placed where the metals are, is a gas and non-metal.

Where are the non-metals found in the periodic table?

The lanthanides and actinides are primarily found at the bottom two detached rows (f-block) of the periodic table, where the lanthanides are the top row, and the actinides are the bottom row.

Where are the lanthanides and actinides found?

s = 2

p = 6

d = 10

f = 14

What are the maximum electrons for all s, p, d, f subshells?

2n², where n is the shell number. (FOR K, L, M, N MAIN ELECTRON SHELLS)

State the rule for finding the maximum amount of electrons per main energy level/electron shell:

Electronic configuration describes how electrons are arranged within the energy shells or orbitals of an atom.

What is electronic configuration?

Electronic structure is the arrangement of electrons in the shells or levels around the nucleus of an atom.

What is electronic structure?

Electrostatic forces are the forces of attraction between small particles with opposite electrical charges.

What are electrostatic forces?

Electron shells are the layers of electrons arranged around the nucleus of an atom.

What are electron shells?

The layers of electrons or electron shells arranged around an atomic nucleus are referred to be at different energy levels.

Define energy levels.

The mass number shows how many protons and neutrons there are in the atom combined.

The atomic number shows how many protons there are. The number of protons is the same as the number of electrons. This is because an atom has no overall charge, so in order to balance these two opposing charges out, the atom must have the same number of protons and electrons.

What does the mass number and atomic number show?

The periodic table is a table of all chemical elements arranged in order of their atomic number.

What is the periodic table?

Across a period: Decreases

• This is because as you go across from left to right on a period, the positive nuclear charge increases as the atomic number increases, the increased nuclear charge pulls electrons closer to the nucleus and makes the atom smaller as no electron shells are added, and the electrons are more attracted to the nucleus.

Down a group: Increases

• This is because as you go down a group, more electron shells are added, increasing the size of the atom and thus the atomic radius.

State the trend for atomic radius in the periodic table.

Across a period: Increases

• This is because the positive nuclear charge increases as you go across a period and there are no new electron shells being added and increasing the size of the atom.

• The shielding effect is relatively constant and the distance between the nucleus and the electrons are smaller because of the increased attraction.

• The electrons become very hard to remove due to these reasons and thus the ionization energy increases.

Down a group: Decreases

• More electron shells are added, increasing the distance between the electrons and the nucleus of the atom.

• This increased distance leads to a weaker attraction.

• The shielding effect is much greater due to the greater distance, so the electrons have an even weaker attraction.

• The weaker attraction leads to the electrons being very easy to remove, so thus the ionization energy decreases.

State the trend for ionization energy in the periodic table.

Across a period: Increases

• The positive nuclear charge increases as you go across a period and so the attraction is much larger and stronger.

• The shielding effect is relatively constant, and so the electrons are held more tightly in the bond.

• The atomic radius decreases as you go across a period, so the electrons are held closer and more tightly.

Down a group: Decreases

• The atomic radius increases and the atom has more electron shells added to it, increasing its distance between the nucleus and the electrons.

• The electrons have a greater shielding effect on them, decreasing their attraction and making it hard for the atom to attract the electrons in the bond strongly.

State the trend for electronegativity in the periodic table.

GROUP 1 ALKALI METALS:

• The boiling and melting points decrease as you go down the group.

• REASON: This is because the metallic bonds decrease as you go down, and the atomic radius increases (so the attraction is weaker and bonds are weaker).

GROUP 7 + 8 (periodic table 17 and 18) HALOGENS & NOBLE GASES:

• The boiling and melting points increase as you go down the group.

• REASON: This is because the intermolecular forces increase as you go down the group, and these forces require a huge amount of energy to overcome, so thus the boiling and melting points are very high.

State the trend for melting and boiling points in the periodic table.

Down a group: Increases

Across a period (LEFT TO RIGHT): Decreases

Across a period (RIGHT TO LEFT): Increases

Up a group (BOTTOM TO TOP): Decreases

State the trend for metallic character in the periodic table.

Electronegativity measures how strongly an atom can attract electrons in a bond.

Define electronegativity.

Ionization energy is the energy needed to remove an electron from an atom.

Define ionization energy.

Alkali metals are alkaline elements found in group 1 of the periodic table. They have one valence electron in their outermost electron shell, and form alkaline solutions with water. They are very reactive with water and air, and have to be kept under oil to prevent reacting with them.

• Alkali metals FORM alkaline solutions.

Define Alkali Metals (GROUP 1):

Halogens are very reactive non-metals, that have 7 valence electrons in their outermost electron shell, since atoms all strive for stability, they are very reactive as they really want to fill up their electron shell with the missing 1 electron.

They are salt formers as halo means salt, and gen means to produce in Greek.

• Halogens means “salt formers”.

Define Halogens (GROUP 17):

Nobles gases are unreactive or inert gases. This is because they have a full outermost electron shell with 8 valence electrons. They are very stable, and have no need to fill up their electron shell, so thus they are very unreactive and that is where their namesake comes from.

They rarely react with anything, just like how nobles don’t mix with the commoners.

• Noble gas → from noble, unreactive. Used to be called inert gases until calling them noble gases became popularized.

Define Noble Gases (GROUP 18):

Transition metals are metals found in groups 3-12. They are called transition metals because their atoms can have partially filled d-orbitals, letting them change between multiple oxidation states (different charges). They are also found in the transition zone (between metals on the left and non-metals on the right).

• Transition metals are found in the transition zone.

Define transition metals (GROUPS 3-12, D-BLOCK):

s = Groups 1 and 2. (two groups = max 2 electrons)

p = Groups 13 to 18 (6 groups = max 6 electrons)

d = Groups 3- 12 (10 groups = max 10 electrons)

f = Lanthanides and Actinides, 14 groups. (14 groups = max 14 electrons)

Where are the s, p, d, f blocks located on the periodic table?

IUPAC Stands for the International Union of Pure and Applied Chemistry.

What is IUPAC?

There are 7 periods and 18 groups, with 118 elements.

How many groups and periods are there in the periodic table?

Aufbau’s principle is a law that states that electrons first fill up the lowest energy levels before filling up higher energy levels. This law helps us predict the electronic configuration of an atom, and how electrons are distributed in their shells.

What is Aufbau’s Principle?

• Ends with -ide.

• Ends with -ate or -ite if there is oxygen as a third element.

• Ending with -ide means its a salt usually.

• Ionic compounds are formed from a metal and a non-metal.

Rules for naming ionic compounds?

• Ends with - ide

• Ends with -ate or -ite if it contains oxygen as a third element

• Start with these plural markers to show that the element has these many atoms (for the first element, no need to put in mono- if it has only one atom, you have to for the second though.)

  1. Mono-

  2. di-

  3. tri-

  4. tetra-

  5. penta-

  6. hexa-

  7. hepta-

  8. octa-

  9. nona-

  10. deca-

Rules for naming covalent compounds?