Chemistry Test #1 Flashcards
(31 cards)
How many valence electrons do elements in group 14 have?
4 valence electrons.
Define valence electrons.
The electrons found on the outermost energy level of an atom and are responsible for determining the atom’s chemical properties.
Transition metals are found in:
Groups 3-12
What are transition metals characterized by?
Their ability to form stable ions with various oxidation states due to the presence of incompletely filled d orbitals.
How many electrons can the p sub level hold?
A maximum of 6 electrons. According to the Pauli exclusion principal, there are three orbitals each capable of accommodating up to 2 electrons.
The F-Block is characterized by….
filling the 4f sub level. The sub level is found within the lanthanide and actinide series and can hold a maximum of 14 electrons.
Elements in group 16 have ____ electrons in their outermost energy level.
6 electrons.
Elements in the D-Block are often referred to as…
transition elements. These element exhibit variable oxidation states and form colorful compounds due to the presence of partially filled d orbitals.
How many electrons can the d Sublevel hold?
A maximum of 10 electrons. (this sub level consists of 5 orbitals, each capable of holding up to 2 electrons)
what block are Lanthanides and Actinides located?
The F-block of the periodic table. (This series of elements are characterized by the filling of the 4f and 5f orbitals)
How many valence electrons do elements in the halogen group typically have?
7 valence electrons.
How does the atomic radius size trend?
The atomic radius increases from top to botton within a group in the periodic table. (this trend occurs because the outermost electrons are in higher energy levels- leading to larger atomic sizes)
The radius of an atom decreases when it…
Loses an electron. (this occurs because the removal of an electron reduces the repulsion between electrons in the outer energy levels, causing the remaining electrons to be pulled closer to the nucleus)
The radius of an atom increases when it…
Gains an electron. (the addition of an electron leads to increased electron-electron repulsion, causing the outermost electrons to occupy a larger volume)
What is ionization energy?
the energy required to remove an electron from an atom
What is the trend in Ionization Energy?
The trend in ionization energy generally increases fro left to right across a period in the periodic table due to increased nuclear charge.
What is the octet rule?
The octet rule states that atoms tend to gain, lose, or share electrons with other atoms to achieve a full octet of valence electron, thereby attaining greater stability.
What is the definition of electronegativity?
Electronegativity a measure of an atoms ability to attract shared electrons in a chemical bond.
Salts with metals are typically formed by elements belonging to which group?
The Alkali metals (alkali metals typically form ionic compounds with nonmetals, resulting the formation of salts.
What properties do metalloids exhibit?
They have properties intermediate between metals and nonmetals, useful in various technological applications.
What characteristic is shared by all noble gases?
They all have full valence electron shells, making noble gases stable and uncreative under normal conditions.
What characteristic group are Magnesium and Calcium in?
Alkaline Earth Metals. These metals are characterized by their reactivity forming basic oxides and hydroxides.
Describe 3 physical properties of liquid nitrogen.
inert, colorless, odorless, noncorrosive, nonflammable, and extremely cold
Explain how liquid nitrogen’s properties arise from tis molecular structure and intermolecular forces.
Nitrogen gas (N2) is diatomic and nonpolar due to its linear molecular structure, resulting in weak intermolecular forces known as London dispersion forces.
