Flashcards in Chapter 4 Deck (51):
1
Two non-metals combine to form what?
a covalent compund
2
A metal and a non-metal combine to make what?
a binary salt
3
a metal oxide and a non-metal oxide combine to form what?
ternary salt
4
A metal oxide and water combine to create what?
a base
5
A non-metal oxide and water combine to form what?
an acid
6
def. A rapid and exothermic reaction between oxygen and a fuel, producing carbon dioxide
and water, along with other oxides, depending on the composition of the fuel
Combustion
7
def. Describes a process that absorbs energy from the surroundings, most commonly in the
form of heat and/or light
endothermic
8
def. A single compound breaks apart, or decomposes, into two or more chemical species
Decomposition
9
def. The minimum energy required to start a chemical reaction
Activation energy
10
def. Describes a process that releases energy to the surroundings, most commonly in the
form of heat and/or light
exothermic
11
Forming chemical bonds _________ energy to the surroundings
releases
12
Breaking chemical bonds ________ energy
absorbs
13
def. Two or more chemical species combine to form a single compound
Synthesis
14
def. A reaction between a compound and an element in which the element replaces an
element of the same type in the compound, creating a different compound and a different element
Single Replacement
15
def. A ranking of elements according to their reactivities, from most to least reactive
Activity Series
16
The more reactive an element is the ______ likely it is to form a compound
more
17
def. A reaction between two compounds that trade cations (or trade anions) between them
Double Replacement
18
what are three types of double replacement reactions?
- precipitation
- neutralization
- gas formation
19
def. A double replacement reaction between two soluble salts, forming two new salts, one
of which is insoluble, creating a precipitate
Precipitation
20
def. An exothermic double replacement reaction between an acid and a base that always
produces a salt and water
Neutralization
21
AB(aq) + CD(aq) becomes AD(aq) + CB(s)
preciptation
22
HX(aq) + MOH(aq) becomes MX(aq) + H2O(l) + heat
neutralization
23
def. An exothermic double replacement reaction between an acid and a base that always
produces a salt and water
Neutralization
24
def. A double replacement reaction that forms an unstable product which spontaneously
decomposes to a gas and water
Gas formation
25
in a _________ : reaction product spontaneously decomposes
to a gas and water, creating three products
gas formation
26
acid + base becomes salt + water
neutralization
27
in a ________ :one product is soluble, other is an insoluble
precipitate
precipitatiion
28
in a _____ : Fuel + oxygen becomes carbon dioxide + water
combustion
29
when does a single replacement occur?
Replacement only occurs if the incoming element is more reactive than
the element it will replace in the compound
30
def. A diagram showing how potential energy changes from reactants to products, allowing you to better understand the characteristics of a given reaction
Potential energy diagram
31
What does enthalpy describe?
the total internal energy in a system
32
Can you measure the total energy of a system?
No
33
def. a measure of how much energy a chemical process converts between heat and potential energy
change in enthalpy (ΔH)
34
What's the formula for change in enthalpy?
ΔH = Hproducts–Hreact
35
A negative change in enthalpy signifies what kind of system?
Exothermic
36
A positive change in enthalpy signifies what kind of system?
endothermic
37
def. Forces that exist between individual molecules, either attracting them together, or repelling them apart
Intermolecular forces
38
Changes in __________ forces produce changes in physical form, like changes of state and dissolution, as particles move further apart or closer together
intermolecular
39
def. Attractive forces that exist within a molecule or compound, holding the atoms together (Really just a broader, more general term for chemical bond)
Intramolecular forces
40
Changes in ________ forces produce chemical changes, as existing bonds break and new bonds form, resulting in new and different products
Intramolecular
41
def. One way to measure the strength of a chemical bond, representing the amount of energy released when a bond forms and the amount needed to break it (The higher the bond energy, the stronger the bond)
Bond Energy
42
Once started ________ reactions are self-sustaining , as some of the energy they release provides the energy required for more reactant to reach the activation energy?
Exothermic
43
___________ reactions never have enough energy to reach activation energy on their own, and therefore require a constant input of energy to both start them and maintain their progress
Endothermic
44
def. Any reaction that starts automatically upon mixing the reactants, without the need to add any additional energy to reach activation energy
Spontaneous reaction
45
What two things influence reaction rate?
Catalysts and temperature
46
Both catalysts and an increase in temperature make it _______ for the reactants to reach activation energy, making the reaction easier and the rate ________
easier, faster
47
def. A balanced chemical equation that includes energy as if it were a reactant or a product
Thermochemical equation
48
In an endothermic reaction, energy acts like _____
a reactant
49
in an exothermic reaction, energy acts like a _______
product
50
change in enthalpy is an ________ property
extensive
51