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Marine Chemistry > Chemical Bonding Part 1 > Flashcards

Chemical Bonding Part 1 Flashcards

1
Q

Electronegativity

A

atoms relative ability to attract/pull on electrons while bonded

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2
Q

Ion

A

atoms with a charge of either positive or negative charge

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2
Q

Cation

A
  • an atom that has lost electrons
  • has a positive charge
  • are mostly metals
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3
Q

Anion

A
  • an atom that has gained electrons
  • has a negative charge
  • are mostly nonmetals
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4
Q

Covalent bond

A
  • Sharing of electrons
  • Attraction of nucleus to another atoms electrons
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4
Q

Ionic bond

A
  • transfering/stealing of electrons
  • Comes from the word ion
  • Attractions of oppositely charged ions
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5
Q

Polar covalent bond

A
  • electrons shared unequally
  • unequal distribution of energy
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6
Q

Nonpolar covalent bond

A
  • electrons shared equally
  • equal distribution of energy
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7
Q

Formula unit

A
  • the simplest combination of ions that make a neutral compound
  • corresponds with a chemical formula
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8
Q

Ionic compound

A
  • a compound made up of positive and negative ions whose charges add to zero
  • electrons gained = electrons lost
  • they are often binary
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9
Q

Lattice energy

A
  • energy released when 1 mole of an ionic crystalline compound is formed from separate atoms
  • Unit: kJ/mol or J/mol
  • lattice energy is always (-) b/c that means energy that is released
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10
Q

Polyatomic ion

A
  • molecules with an overall net charge
  • atoms are bonded covalently but the atoms have picked up or lost electrons along the way
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11
Q

Oxyanion

A
  • negatively charged polyatomic ions containing oxygen
  • (-ate/-ite) -ate will always have 1 more oxygen than -ite
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12
Q

Molecular mass

A
  • the mass of one molecule
  • used for covalent bonding
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13
Q

Molar mass

A
  • the mass of one molecule
  • used for covalent bonding
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13
Q

Formula mass

A
  • the mass of a single formula unit
  • measured in AMU
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14
Q

Percent composition

A
  • The percentage of the compound that is made up of a certain element
  • the part element divided by the total compound times 100
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15
Q

Periodic trend for electronegativity and why

A
  • Increases across periods
  • Greater nuclear charge and a smaller radius across periods.
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16
Q

Group trend for electronegativity

A
  • Decreases down groups/families
  • Larger radius and shielding effect(weaker pull)
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17
Q

what are the two main types of bonding?

A

covalent and ionic bonding

18
Q

Explain in depth, ionic bonding

A
  • a transfer of electrons
  • one is stealing electrons from another
  • between nonmetals and metals
  • metal loses electrons as they are weaker and the nonmetals gain electrons as they are the stronger ones.
19
Q

Explain in depth, covalent bonding

A
  • sharing of electrons
  • none gain or lose electrons but one can have more pull than another
  • between two nonmetals where they both want to share extra electrons
  • if they are equally shared, it is nonpolar but if they are unequally shared, it is polar.
20
Q

How do you use EN difference to predict type of bond?

A
  • Between two elements, you must find the difference between their electronegativities.
20
Q

If the difference is greater than 1.7, then it is…

A

an ionic bond

21
Q

If the difference is less than 1.7 but greater than 0.3, then it is a…

A

polar covalent bond

21
Q

If the difference is greater than 0 but less than 0.3, then it is a…

A

nonpolar covalent bond

22
Q

how do ionic bonds form?

A
  • First, one atom steals electrons from another
    *Now the atoms are no longer neutral and the oppositely charged ions attract.
  • Then, the charged ions attract to form an ionic bond.
23
Q

How do you use electron configuration and octet rule to predict how ionic compounds will form?

A
  • You can figure out how many valence electrons with it
  • If the element has 1-3 VE, then they will lose electrons and have a positive charge
  • If the element has 5-7 VE, then it will gain electrons and have a negative charge
  • If there are 4 VE, the element has to choose to lose/gain 4 valence electrons depending on the other element.
24
Q

Why we don’t describe ionic compounds in terms of molecules?

A
  • They are formed from their big differences in electronegativities
  • Covalent compounds form molecules
24
Q

What holds ionic bonds together?

A
  • The form from the attraction between ions
  • The negative and positive charges attract to each other, holding the ions together
25
Q

How do you write chemical equations to describe ionic bonding?

A
  • You start off by writing the simplest drawing of the compound, with the charges too
  • Then, you make it by adding a plus sign
  • After that, you add subscripts with charges
  • Finally, you make the equation with just the element’s symbol and subscript, no charge.
26
Q

How/why ionic compounds form a crystal lattice?

A
  • Ionic compounds form a crystal lattice by holding all the ions together b/c they are oppositely charged
  • The shape is then determined by the ratio of ions and the size of ions
27
Q

How does lattice energy relate to various properties of ionic compounds?

A
  • When the lattice energy –> higher, it causes ionic compounds to change.
    *Substance becomes harder
    *Has a higher melting point
    *Has a higher boiling point.
28
Q

Names and formulas of common polyatomic ions

A

Ammonium: NH4+1
Hydronium: N3O+1
Nitrite: NO2-1
Nitrate: NO3-1
Chlorite: ClO2-1
Chlorate: ClO3-1
Perchlorate: ClO4-1
Hypochlorite: ClO-1
Hydroxide: OH-1
Cyanide: CN-1
Carbonate: CO3-2
Hydrogen Carbonate: HCO3-1, Hydrogen Sulfate: HSO4-1
Sulfite: SO3-2
Sulfate: SO4-2
Peroxide: O2-2
Chromate: CrO4-2
Phosphate: PO4-3
Acetate: C2H3O2-1

29
Q

How to write chemical formulas for ionic compounds

A
  • First, figure out the symbol for the element
  • Then, figure out the VE of the elements to find the charge
  • After that, if they equal each other out, then you keep them and add nothing
    *On the other hand, if they are unequal, you figure out how much of each element is needed to make it equal
    *Then for the subscript, you put how much of that element you added
30
Q

How to name ionic compounds

A

Rule 1:
* Always put the cation first and anion second
* Put subscripts to show how many of each element there is
* If there is more than one polyatomic ion, use parentheses and a subscript to show how many.
Rule 2:
* If the cation is a transition metal, tin, or lead, you write its charge in a roman numeral in parentheses * To write the name of the anion, if it is a monatomic ion, then change the ending to “ide”
* If the anion is polyatomic, the ending stays the same.

31
Q

How to convert between moles, grams and formula units for ionic compounds

A

Mass(g) –> moles: divide by the molar mass
Moles –> mass(g), multiply by molar mass
Moles –> atoms, divide by avogadro’s number
Atoms –> moles, multiply by avogadro’s number

32
Q

How to calculate percent composition WITHOUT lab data

A
  • Find the element’s atomic masses on the periodic table
  • Then, add them together, all of the elements, to find out the total mass of the compound
  • After, do the rest normally by putting the element over the compound to find the percent composition.
33
Q

How to calculate formula mass

A

Take the atomic masses of each other and the elements in the equation and add them all together. In the end, put AMU as the unit for formula mass.

34
Q

How to calculate molar mass

A

Take the mass of each molecule and add it together. So, the mass of one molecule as a whole number.

35
Q

why can’t you calculate molecular mass for NaCl and what can you of instead?

A
  • You would use formula mass
  • These compounds form crystal lattice, not molecules
36
Q

what happens when lattice energy is released?

A
  • makes bond more stable
  • potential energy goes down
37
Q

atoms bond to become more stable which lowers their what?

A

potential energy

38
Q

ionic bonding on main group elements

A
  • s + p blocks
  • charges are consistent
    *
39
Q

ionic bonding on transition/inner transition elements

A
  • charges vary
  • always cations(lose electrons)
  • all have 2 VE
40
Q

common properties of ionic compounds

A
  • hard to the touch
  • brittle
  • high melting/boiling point
  • dissolve in water
41
Q

how to break ionic compounds

A
  • lots and lots of energy needed
  • dissolving in water too
    *good conductors of electricity
42
Q

what is the formula for percent composition

A

(part of compound/total compound) x 100

Marine Chemistry (11 decks)

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