Unit 2: Periodic Table Flashcards
(28 cards)
What are the three states of matter that elements can exist? Examples?
➡️Gas: oxygen, nitrogen
➡️liquid: Mercury
➡️solid: copper
How did Mendeleev organize his elements? What was the underlying pattern?
➡️Organized his elements in columns,families/groups, and rows,periods.
➡️Rows and columns are based upon similar chemical traits and properties
↪️discovered repartition among properties and created the periodic table through the observations
Why did Mendeleev leave gaps in his table? Did the gaps resolve?
➡️Gaps were left in the table because he predicted more elements were going to be found.
➡️Gaps were resolved and and Mendeleev’s predictions were correct. There are now 9⃣ basic element groups.
How was the periodic table organized?
By increasing atomic mass
Metal
➡️elements that can be thinned out and hammers and still retain its toughness
↪️elements that give up their electrons easily and carry electricity well
(Left side of periodic table)
➡️malleable
➡️ductile
Nonmental
➡️right side of periodic table
➡️accept electrons easily but do NOT hold electricity well
↪️accept electrons to complete octet
Transition Metals
➡️occupy groups 3⃣ through 1⃣2⃣ on periodic table
➡️D block or F block elements because they are known for filling the d and f orbitals
Metalloid
➡️between metals (on left) and nonmetals (on right) on periodic table
↪️7⃣ total
➡️exhibit the same characteristics of metals and nonmetals
Alkali Metals (group 1)
➡️ contain 1 valence electron, making them very reactive
➡️quickly combines with oxygen and water causes powerful reaction
Alkaline Earth Metals (group 2)
➡️two valence electrons causing the metals to be highly reactive (lose their electrons during chemical reactions)
➡️behavior can be easily predicted
↪️form weak bases when in contacted with water; with oxygen form oxides that cause high melting points.
Halogens (group 17)
➡️ 7 valence electrons; very reactive (need one more electron to make stable)
➡️ easily bonds with Alkali Metals (group 1)
➡️when reacts with metals, salt is produced
➡️only group w/ elements commonly found in each state of matter
Noble Gases (group 18)
➡ unreactive because they contain a “stable set of valence electrons p)
➡️typically seen as monatomic (single atom) elements -> low boiling
➡️gas state;small % of Earth’s atmosphere
Lanthanide Series (separate section; inner transition metals)
➡️atomic # fall within transition metals
➡️commonly occurs in nature, mixed “rare earth metals”
➡️difficult to separate inner metals in pure elements form
Actinide Series (Period 7)
➡️unstable because most were combined in a laboratory
➡️all radioactive
➡️only three (3) metals occur naturally in this series
Cation
➡️a type of ion that has more protons than electrons causing it to have a net positive charge
➡️forms when an atom loses one or more valence electrons
↪️atoms of metals
Anion
➡️negatively charged ion
➡️forms when an action GAINS one or more valence electrons
↪️atoms of nonmetals
Ion
➡️particle with a charge
↪️gaining or losing electrons
↪️gaining e- produces NEGATIVE from non-metals
↪️losing e- produces POSITIVE from metals and hydrogen
Valence Electrons
➡️Octet Rule
↪️atoms will gain, lose or share electron I’m order to get 8 valence electrons
Isoelectronic
An ion/atom etc. has the same # of electrons as what you are comparing it to.
Ionization Energy
The minimum amount of energy that is required to an electron from an atom
Atomic Radius
The size of an atom from the outside electron orbit to the nucleus.
Electronegativity
The tendency of an atom to attack electrons and acquire a negative charge.
Effective Nuclear Charge
Net positive charge that is felt by an electron in a multi-electron atom.
Electron Shielding
➡️less pull with more layers
➡️answer = depends on the loss/gaining of valence electrons
