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Energy and Chemical Reactions: Terms and Concepts, Quizzes of Chemistry

Definitions and explanations for various terms related to energy and chemical reactions. Topics include potential and kinetic energy, energy units, bond dissociation energy, heat of reaction, endothermic and exothermic reactions, activation energy, transition state, reaction rate, catalysts, and intermolecular forces. Students of chemistry will find this document useful for understanding the fundamental concepts of energy and chemical reactions.

Typology: Quizzes

2012/2013

Uploaded on 12/07/2013

sydneyc33
sydneyc33 🇺🇸

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TERM 1
energy
DEFINITION 1
the capacity to do work
TERM 2
potential energy
DEFINITION 2
stored energy
TERM 3
kinetic energy
DEFINITION 3
energy of motion
TERM 4
energy is measured in ____
DEFINITION 4
calories and joules
TERM 5
I Cal
DEFINITION 5
nutritional calorie
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energy

the capacity to do work

TERM 2

potential energy

DEFINITION 2

stored energy

TERM 3

kinetic energy

DEFINITION 3

energy of motion

TERM 4

energy is measured in ____

DEFINITION 4

calories and joules

TERM 5

I Cal

DEFINITION 5

nutritional calorie

when a bond is formed, energy is _____

released

TERM 7

when a bond is broken, energy is _____

DEFINITION 7

added

TERM 8

heat of reaction

DEFINITION 8

the energy absorbed or released in any reaction

enthalpy change

TERM 9

when energy is absorbed, reaction is _____

DEFINITION 9

endothermic

TERM 10

when energy is released, reaction is ____

DEFINITION 10

exothermic

when ^H is

positive

more energy is needed to break bonds than is released

from forming bonds

bonds broken in reactants are stronger than bonds

formed in products

reaction is endothermic

heat is absorbed

TERM 17

Ea

DEFINITION 17

activation energybarrier separating reagents and products

TERM 18

when Ea is high

DEFINITION 18

large barrier for reagents to be converted to products

slow reaction

few molecules have enough energy to reach the energy

barrier

TERM 19

when Ea is low

DEFINITION 19

more molecules are able to cross the energy barrier and

form products

faster reaction

TERM 20

^H

DEFINITION 20

the difference in energy of reagents and products

doesn't depend on Ea

energy of products - energy of reagents

transition state

at top of Eatransition between reactants and productsbond is

partially broken and partially formed

TERM 22

increase concentration

DEFINITION 22

increase reaction rate

TERM 23

increase temperature

DEFINITION 23

increase reaction rateincrease kinetic energy

TERM 24

catalyst

DEFINITION 24

a substance that speeds up the rate of a reaction by lowering

the activation energy

TERM 25

enzymes

DEFINITION 25

biological catalyst

removing reagent

> reagents

TERM 32

adding product

DEFINITION 32

> reagents

TERM 33

removing product

DEFINITION 33

> products

TERM 34

increasing temperature

DEFINITION 34

endothermic > productsexothermic > reagents

TERM 35

decreasing temperature

DEFINITION 35

endothermic > reagentsexothermic > products

increasing pressure

> side with fewer moles

TERM 37

decreasing pressure

DEFINITION 37

> side with more moles

TERM 38

k=

DEFINITION 38

pressure times volume

TERM 39

boyle's law

DEFINITION 39

for a fixed amount of gas at a constant temperature, the

pressure and the volume of a gas are inversely

relatedp1v1=p2v

TERM 40

charles' law

DEFINITION 40

for a fixed amount of gas of constant pressure, the volume of

a gas is proportional to its temperature in KelvinV1 = V2T

T

standard temperature

273 K or 0C

TERM 47

standard molar volume

DEFINITION 47

22.4 L

TERM 48

ideal gas law

DEFINITION 48

PV = nRT

TERM 49

intermolecular forces

DEFINITION 49

the attractive or repulsive forces that exist between

molecules

TERM 50

London dispersion forces

DEFINITION 50

the weak interactions due to momentary changes to electron

density of a molecule

all covalent molecules have this

the larger the molecule, the ___ the attractive

forces between the 2 molecules

larger

TERM 52

dipole dipole interactions

DEFINITION 52

the attractive forces between the 2 permanent dipoles of 2

polar molecules

molecules must be polar

TERM 53

hydrogen bonds

DEFINITION 53

the interaction between a hydrogen atom bonded to an O an

N or an F, or an O,N, or F on another molecule

high electronegativity

strongest bond

TERM 54

the stronger the intermolecular forces, the

____ the boiling and melting points

DEFINITION 54

higher

TERM 55

vapor pressure

DEFINITION 55

the pressure exerted by gas molecules in equilibrium with

the liquid phase

molecular solid

composed of individual molecules arranged regularly

TERM 62

network solid

DEFINITION 62

composed of a vast number of atoms covalently bonded

together forming sheets or 3D arrays

TERM 63

metallic solid

DEFINITION 63

a lattice of metal cations surrounded by a free moving cloud

of electrons

TERM 64

crystalline solid

DEFINITION 64

regular arrangement of particles with a repeating structure

TERM 65

amorphous solid

DEFINITION 65

no regular arrangement of its closely packed particles

heat of

fusion

the amount of energy needed to melt 1gram of a substance

TERM 67

heat of vaporization

DEFINITION 67

the amount of energy needed to vaporize 1 gram of a

substance