Back to AI Flashcard MakerBiochemistry /Atomic Structure and Periodic Properties Part 2

Atomic Structure and Periodic Properties Part 2

Biochemistry40 CardsCreated 4 months ago

This deck covers key concepts related to atomic structure and periodic properties, including definitions, electron configurations, bond types, and more.

What is the definition of isoelectronic?

species with identical electron configurations to the noble gas to the right
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Key Terms

Term
Definition
What is the definition of isoelectronic?
species with identical electron configurations to the noble gas to the right
What is the ionic radius?
radius of a cation or an anion
What happens to the radius when an atom loses an electron to become a cation?
the radius decreases due in part to a reduction in electron-electron repulsions in the valence shell.
What happens to the radius when an atom gains one or electrons to become an anion?
the radius increases due in part to a increased electron-electron repulsions.
What is an isoelectronic series?
series of 2 or more species that have identical electron configurations but different nuclear charges. ex: O2-, F-, Ne
How many valence electrons do the alkaline earth metals possess?
2 electrons

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TermDefinition
What is the definition of isoelectronic?
species with identical electron configurations to the noble gas to the right
What is the ionic radius?
radius of a cation or an anion
What happens to the radius when an atom loses an electron to become a cation?
the radius decreases due in part to a reduction in electron-electron repulsions in the valence shell.
What happens to the radius when an atom gains one or electrons to become an anion?
the radius increases due in part to a increased electron-electron repulsions.
What is an isoelectronic series?
series of 2 or more species that have identical electron configurations but different nuclear charges. ex: O2-, F-, Ne
How many valence electrons do the alkaline earth metals possess?
2 electrons
A cation of +2 indicates that an element has?
lost 2 electrons
For a particular element, identify the species that has the smallest radius A. radical B. anion C. cation D. neutral
C. cation
Identify the elements correctly show by decreasing radii size. A. N3- > N B. Cu2+ > Cu+ C. K+ > K D. N> N3-
A. N3- > N
Place the following in order of increasing first ionization energy. N, F, As
As, N, F
Give the electron configuration for O
1s2 2s2 2p4
Of the following, which atom has the largest atomic radius? A. Li B. Na C. F D. Cl
B. Na
Place the following in order of decreasing magnitude of lattice energy K2O, Rb2S, Li2O
Li2O, K2O, Rb2S
Identify the weakest bond A. Double covalent bond B. triple covalent bond C. single covalent bond
C. single covalent bond
Give the number of valence electrons for XeI2
22 valence electrons
A reaction is exothermic when: A. weak bonds break and strong bonds form. B. weak bonds break and weak bonds form. C. strong bonds break and weak bonds form. D. strong bonds break and strong bonds form
A. weak bonds break and strong bonds form.
Identify an ionic bond: A. electrons are pooled B. electrons are transferred C. electrons are shared D. electrons are lost
B. electrons are transferred
Identify a bond with covalent bonding A. KBr B. K C. H2Se D. Ne
C. H2Se
What is the Lewis Theory?
simplest bonding theories emphasizes valence electrons to explain bonding using lewis we can draw models called lewis structure
What do lewis structures allow us to predict?
molecular stability, shape, size, and polarity
Why do chemical bonds form?
chemical bonds form because they lower the potential energy between the charged particles that compose atoms.
What types of atoms make up an ionic bond?
metal and nonmetal electrons transferred NaCl
What type of atoms make up a covalent bond?
nonmetal and nonmetal electrons shared H2O
What type of atoms make up a metallic bond?
metal and metal electrons pooled Sodium Metal, Na(s)
What happens when a metal atom loses electrons?
it becomes a cation
What happens a nonmetal gains electrons?
it becomes an anion nonmetals have high ionization energies (difficult to remove electrons)
How many valence electrons do transition metals have?
Two valence electrons
Metals form _____ by losing valence shell electrons Non metals form ______ by gaining valence electrons
CATIONS ANIONS
For main group metals, the number of dots indicates:
the number of electrons that are lost
For nonmetals in the second period, the number of unpaired dots indicates:
the number of bonds the atom can form
What is lattice energy?
amount of energy required to convert a mole of ionic solid to its constituent ions in the gas phase estimates the strength of bonds in an ionic compound. always exothermic
What is electronegativity?
The ability of an atom to attract bonding electrons to itself increases across period (left to right) decreases down group (top to bottom)
If the difference in electronegativity between bonded atoms is 0, what type of bond is it?
Pure covalent
If the difference in electronegativity between bonded atoms is between .1-.4, what type of bond is it?
Non polar covalent
If the difference in electronegativity between bonded atoms is .5-1.9, what type of bond is it?
polar covalent
If the difference in electronegativity between bonded atoms is 2.0 or greater, what type of bond is it?
100% ionic
What is dipole moment?
measure of bond polarity material with a + and - end
What is formal charge?
Fictitious charge assigned to each atom in a lewis structure that helps us to distinguish among competing lewis structures.
What is the sum of all formal charges in a molecule?
0
What is bond energy?
The amount of energy it takes to break one mole of a bond in a compound always positive, endothermic