Chapter 5 key terms Flashcards

1
Q

What is electrostatic potential energy?

A

the amount of work done to move a unit charge from a reference point to a specific point inside the field without producing an acceleration

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2
Q

When does electrostatic occur?

A

seen between oppositely charged ions

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3
Q

Is energy released or consumed when chemical bonds are formed?

A

released

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4
Q

What is the relationship between potential energy and the distance of ions from one another?

A

As Ions become closer, potential energy decreases

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5
Q

Is energy consumed or released when chemical bonds are broken?

A

consumed

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6
Q

What is an open system?

A

a region that can exchange heat and mass with its surroundings

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7
Q

What is a closed system?

A

a region that can only exchange heat with its surroundings

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8
Q

What is an Isolated system?

A

a region that can’t exchange heat or mass with its surroundings

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9
Q

Is delta E positive or negative when the system gains energy from the surroundings?

A

positive

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10
Q

Is delta E positive or negative when the system loses energy to the surroundings?

A

negative

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11
Q

Meaning of +q and - q

A

+q: system gains heat
-q: system loses heat

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12
Q

Meaning of +w and -w

A

+w: work done on the system
-w: work done by system

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13
Q

meaning of +deltaE and -deltaE

A

+deltaE: net gain of energy by system
-deltaE: net loss of energy by system

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14
Q

What’s an endothermic process?

A

heat is absorbed by the system from the surroundings

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15
Q

What’s an exothermic process?

A

heat is released by the system into the surroundings

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16
Q

At constant pressure what is enthalpy?

A

the heat gained or lost

17
Q

Is deltaH positive or negative in an endothermic process?

A

positive

18
Q

Is deltaH positive or negative in an exothermic process?

A

negative

19
Q

What does enthalpy change for a reaction depend on?

A

the states of the reactants and the products

20
Q

What is bond enthalpy?

A

the enthalpy associated with breaking one mole of a particular bond in a gaseous substance

21
Q

Can bond enthalpy be negative?

A

No, its always positive because energy is required to break chemical bonds