Chem lecture homework notes !
Isotopes are atoms of the same element that have the same _____ number but a different _____
number. This is because isotopes have the same number of protons but a different number of
_____. Atomic, mass, neutrons !
Same column (group)- similar electronic and chemical properties!
Same row (period) -similar size!
Each element has a unique number of _____, which is called its atomic number. In an
uncharged atom, this number is also equal to the number of _____ present.!
Protons, electrons!
Which of the following can contain a maximum of 2 electrons? (Select all that apply.)!
The 1s orbital!
A 2p orbital!
The first shell!
Atoms bond in order to achieve a full shell of _____ electrons, leading to a system that has
_____ energy and increased stability, compared to the unbonded atoms.!
valence; decreased!
Which of the following statements correctly describe the atomic number of an element? (Select
all that apply.)!
Each element has a unique atomic number.!
The atomic number is equal to the number of protons in the nucleus.!
Atoms will bond chemically so as to attain a complete outer shell of valence electrons. For
elements beyond the first row of the periodic table, this means attaining!
8!
electrons in the valance shell. By contrast, hydrogen, which is in the first row, will bond so as to
attain a valence shell that contains!
2!
which of the following statements correctly describe s and p orbitals? (Select all that apply.)!
The electrons in a p orbital are filled only after an s orbital in the same shell is filled.!
An s orbital is lower in energy than a p orbital of the same energy level.!
Each orbital can have a maximum of how many electrons?!
2!
Which of the following statements correctly describe a chemical bond? (Select all that apply.)!
Atoms bond to attain a full outer shell of valence electrons.!
A chemical bond leads to increased stability.!
Which of the following statements correctly describe the general rule that governs chemical
bonding? Select all that apply.!
An atom will bond so as to attain a complete valence shell.!
An atom will seek to attain the electron configuration of the nearest noble gas.!
, An element on the far left of the periodic table with an element on the far right#
Ionic bond#
Two elements toward the right-hand side of the periodic table#
Covalent bond!
Sodium chloride (NaCl) is an ionic compound. Which of the following statements correctly
describe the bonding in NaCl? (Select all that apply.)!
Na loses an electron to form the cation Na+.!
The electrostatic attractive force between Na+ and Cl- ions defines the ionic bond in NaCl.!
Cl loses an electron to form the anion Cl-.!
Compound-may contain either ionic or covalent bonds, or both!
Molecule-contains only covalent bonds !
Lithium bromide (LiBr) is an ionic compound. The metal lithium _____ an electron to form the
cation Li+, while the nonmetal bromine _____ an electron to form the anion Br-. The ions are
held together by a strong _____ attraction in a crystal lattice.!
loses, gains, electrostatic!
Atoms with one, two, three, or four valence electrons#
One, two, three, or four covalent bonds are formed.!
Atoms with five or more valence electrons#
The formula (8$-$number$of$valence$electrons) gives the predicted number of covalent b!
Select all of the statements that correctly describe covalent bonding.!
Covalent bonds generally form between two elements from the same side of the periodic table.!
A single covalent bond comprises two shared electrons.!
Select all statements that correctly describe the normal bonding pattern for a neutral atom of
each element.!
Hydrogen forms 1 covalent bond and has no lone pairs.!
Oxygen forms 2 covalent bonds and has 2 lone pairs.!
Sodium chloride (NaCl) is an ionic compound. Which of the following statements correctly
describe the bonding in NaCl? (Select all that apply.)!
Na loses an electron to form the cation Na+.!
The electrostatic attractive force between Na+ and Cl- ions defines the ionic bond in NaCl.!
Select all statements that correctly describe the typical number of covalent bonds formed by
common neutral atoms.!
Atoms with 3 valence electrons typically form 3 covalent bonds.!
Atoms with 8 valence electrons do not typically form bonds.!
Atoms with 7 valence electrons typically form 1 bond.!
Arrange the steps involved in drawing a Lewis structure in the correct order. Place the first step
at the top of the list and the last step at the bottom of the list.!
1.Count the valence electrons from all atoms, and place the atoms next to each other
according to their usual bonding patterns.!
Isotopes are atoms of the same element that have the same _____ number but a different _____
number. This is because isotopes have the same number of protons but a different number of
_____. Atomic, mass, neutrons !
Same column (group)- similar electronic and chemical properties!
Same row (period) -similar size!
Each element has a unique number of _____, which is called its atomic number. In an
uncharged atom, this number is also equal to the number of _____ present.!
Protons, electrons!
Which of the following can contain a maximum of 2 electrons? (Select all that apply.)!
The 1s orbital!
A 2p orbital!
The first shell!
Atoms bond in order to achieve a full shell of _____ electrons, leading to a system that has
_____ energy and increased stability, compared to the unbonded atoms.!
valence; decreased!
Which of the following statements correctly describe the atomic number of an element? (Select
all that apply.)!
Each element has a unique atomic number.!
The atomic number is equal to the number of protons in the nucleus.!
Atoms will bond chemically so as to attain a complete outer shell of valence electrons. For
elements beyond the first row of the periodic table, this means attaining!
8!
electrons in the valance shell. By contrast, hydrogen, which is in the first row, will bond so as to
attain a valence shell that contains!
2!
which of the following statements correctly describe s and p orbitals? (Select all that apply.)!
The electrons in a p orbital are filled only after an s orbital in the same shell is filled.!
An s orbital is lower in energy than a p orbital of the same energy level.!
Each orbital can have a maximum of how many electrons?!
2!
Which of the following statements correctly describe a chemical bond? (Select all that apply.)!
Atoms bond to attain a full outer shell of valence electrons.!
A chemical bond leads to increased stability.!
Which of the following statements correctly describe the general rule that governs chemical
bonding? Select all that apply.!
An atom will bond so as to attain a complete valence shell.!
An atom will seek to attain the electron configuration of the nearest noble gas.!
, An element on the far left of the periodic table with an element on the far right#
Ionic bond#
Two elements toward the right-hand side of the periodic table#
Covalent bond!
Sodium chloride (NaCl) is an ionic compound. Which of the following statements correctly
describe the bonding in NaCl? (Select all that apply.)!
Na loses an electron to form the cation Na+.!
The electrostatic attractive force between Na+ and Cl- ions defines the ionic bond in NaCl.!
Cl loses an electron to form the anion Cl-.!
Compound-may contain either ionic or covalent bonds, or both!
Molecule-contains only covalent bonds !
Lithium bromide (LiBr) is an ionic compound. The metal lithium _____ an electron to form the
cation Li+, while the nonmetal bromine _____ an electron to form the anion Br-. The ions are
held together by a strong _____ attraction in a crystal lattice.!
loses, gains, electrostatic!
Atoms with one, two, three, or four valence electrons#
One, two, three, or four covalent bonds are formed.!
Atoms with five or more valence electrons#
The formula (8$-$number$of$valence$electrons) gives the predicted number of covalent b!
Select all of the statements that correctly describe covalent bonding.!
Covalent bonds generally form between two elements from the same side of the periodic table.!
A single covalent bond comprises two shared electrons.!
Select all statements that correctly describe the normal bonding pattern for a neutral atom of
each element.!
Hydrogen forms 1 covalent bond and has no lone pairs.!
Oxygen forms 2 covalent bonds and has 2 lone pairs.!
Sodium chloride (NaCl) is an ionic compound. Which of the following statements correctly
describe the bonding in NaCl? (Select all that apply.)!
Na loses an electron to form the cation Na+.!
The electrostatic attractive force between Na+ and Cl- ions defines the ionic bond in NaCl.!
Select all statements that correctly describe the typical number of covalent bonds formed by
common neutral atoms.!
Atoms with 3 valence electrons typically form 3 covalent bonds.!
Atoms with 8 valence electrons do not typically form bonds.!
Atoms with 7 valence electrons typically form 1 bond.!
Arrange the steps involved in drawing a Lewis structure in the correct order. Place the first step
at the top of the list and the last step at the bottom of the list.!
1.Count the valence electrons from all atoms, and place the atoms next to each other
according to their usual bonding patterns.!
