chemical bonds

Question 1

what is a chemical bond? why do they exist?

Answer 1

an intramolecular force that holds together atoms in a molecule or compound
because of attraction between positive nuclei and negative electrons

Question 2

which becomes an anion in an ionic bond? metal or nonmetal

Answer 2

nonmetal

Question 3

which becomes a cation in an ionic bond? metal or nonmetal?

Answer 3

metal

Question 4

ionic bonds occur between _____ and _____ because of differing ______

Answer 4

metals
nonmetals
electronegativities

Question 5

Can cations and anions in an ionic bond be polyatomic?

Answer 5

yes

Question 6

Are there distinct molecules in ionic bonding?

Answer 6

No, there are collections of ions held together by the attraction of their charges.

Question 7

which 7 elements commonly appear in diatomic form?

Answer 7

hydrogen, oxygen, fluorine, bromine, iodine, nitrogen, chlorine
HOFBrINCl
(hoffbrinkle)

Question 8

What trick is used in ionic bonding to determine subscripts?

Answer 8

Switch the number of electrons it takes to get to the desired outcome.
Ex: MgCl2
Magnesium wants to be like Neon, losing two electrons.
Chlorine wants to be like Argon, gaining one electron
so Mg2Cl1
then switch them
so the final result is MgCl2

Question 9

Covalent bonds create stable compounds if….

Answer 9

the sharing of electrons brings a noble gas electron configuration

Question 10

Why do nonmetals form covalent bonds?

Answer 10

Nonmetals have high electronegativity and ionization energy. This is a compromise, so they can try and reach their full octet while not having to lose any electrons.

Question 11

How many electrons does a single covalent bond contain?

Answer 11

2

Question 12

how many electrons in total does a double covalent bond have? a triple covalent bond?

Answer 12

4

6

Question 13

What do the two elements have to be for a covalent bond to form?

Answer 13

Two nonmetals or a nonmetal and a semiconductor

they do not have to be identical

Question 14

What is “metallic bonding”?

Answer 14

When metal atoms bond by sharing electrons in an “electron sea” shared by all the bonded atoms in the structure.

Question 15

What is a single metallic bond?

Answer 15

Trick question - single metallic bonds don’t exist. Metallic bonds are collective by nature.

Question 16

What can’t be nearby for a sea of electrons to form?

Answer 16

An element with high electronegativity (nonmetal) because it will be ready to accept electrons

Question 17

When do metallic bonds occur?

Answer 17

When the coulombic attraction (charge attraction) that keeps atoms bound to the nucleus is weaker than the electron’s energy

Question 18

Can metallic bonds form among elements with higher ionization energies despite their reluctance to give up electrons?

Answer 18

Yes

Question 19

What properties of metals stem from metallic bonds?

Answer 19

Luster (moving electrons absorb and re-emit light), electrical conductivity (moving electrons absorb charge and travel throughout metal), thermal conductivity (moving electrons absorb heat and travel throughout metal), malleability, and ductility.

Question 20

When an atom is gaining electrons, the number of bonds it will make equals the number of _____

Answer 20

electrons it needs to complete its octet

covalent: both atoms gain the electrons
ionic: more electronegative gains electrons

Question 21

When an atom is losing electrons, the number of bonds it will make equals the number of _____

Answer 21

valence electrons that the atom has.

Question 22

How many bonds do hydrogen atoms make?

Answer 22

Always one, whether its in an ionic or covalent compound.

Question 23

How many lone pairs does carbon normally have?

Answer 23

0, carbon almost always has 4 bonds

Question 24

in a lewis structure of a covalent bond, have many valence electrons does one atom have?

Answer 24

valence electrons = number of electron dots+(2*number of bonds the atom has)

Question 25

Are ionic bonds normally represented by Lewis structures?

Answer 25

No - This is because ionic bonds encompass cations and anions held together by the attraction between positive and negative, and do not have actual individual bonds

Question 26

How are ionic bonds represented by lewis structures

Answer 26

The two lewis structures separate but with a charge and a “+” sign
(ex: Li+F -> [Li] + [F]-)