Shared Flashcard Set

Details

Regents Chemistry
Practice Constructed Response
65
Chemistry
11th Grade
01/13/2012

Additional Chemistry Flashcards

 


 

Cards

Term

 

What is the same in an isotope and what is different in an isotope in terms of subatomic particles?

 

Definition

 

Same Protons

 

 

Different Neutrons

Term

What is the charge of the nucleus?

Definition

 

Positive

 

Term

State two major findings about the atom.

Definition

The atom is mostly empty space.

The nucleus is small and positive.

Term
Explain how spectral lines are produced, in terms of electrons.
Definition

 

Electrons fall from the excited to the ground state.

 

Term

In a nuclear reaction mass is always “lost”. Explain this loss of mass.

Definition

Mass was converted to energy.

Term

 

Calculate the average atomic mass of carbon:

 

98% 12C and 2% 14C

 

Definition

 

 (98/100) (12) + (2/100) (14) = 12.04

 

Term
Why would two elements have similar chemical properties?
Definition

Same group.

Same Valence electrons.

Term
Why does the radius increase as you move down a group?
Definition

 

More Shells

 

Term
Describe three properties of metals
Definition

 

good conductor

malleable and ductile

 shiny

Term
Describe three properties of nonmetals
Definition

 

poor conductor

brittle

dull

Term

Which elements lose electrons when forming ions?

What happens to the radius?

Definition

metals

decreases

Term

 

 

Which elements gain electrons when forming ions?

What happens to the radius?

Definition

 

nonmetals

increases

Term
Name the four types of chemical reactions.
Definition

 

synthesis

decomposition

single replacement

double replacement

Term
[image]
Definition

Kinetic Energy Increases

Potential Energy remains the same

Term
[image]
Definition

Kinetic Energy remains the same

Potential Energy Increases

Term

 

How is an ionic bond formed, in terms of electrons?

Definition

 

Electrons are transferred.

Term

 

How is a covalent bond formed, in terms of electrons?

Definition

 

Electrons are shared.

Term

 

What makes a bond more polar, in terms of electronegativity?

Definition

 

Greater difference in electronegativity.

Term

 

What makes a covalent bond polar?

Definition

 

Unequal sharing of electrons.

Term

 

What makes a covalent bond nonpolar?

Definition

 

Equal sharing of electrons.

Term

 

Why is a molecule polar?

(HINT:SNAP)

Definition

 

Asymmetrical.

Term

 

Why is a molecule nonpolar?

(HINT:SNAP)

Definition

 

Symmetrical.

Term

 

List 3 Properties of ionic compounds.

Definition

 

High Melting Point

Strong forces

Conductor only in the liquid phase

Term

 

List 3 Properties of molecular solids(covalent bonds).

Definition

 

Low Melting Point

 Weak forces

Poor Conductor

Term

 

List 3 Properties of metallic solids.

Definition

 

High Melting Point

Strong forces

Great Conductor

Term

 

What makes a good conductor(in terms of particles)?

Definition

 

Mobile Particles.

Term

 

How do you increase the solubility of a solid in a liquid?

Definition

 

Raise temperature

Term

 

How do you increase the solubility of a gas in a liquid?

Definition

 

Lower temperature

Increase pressure

Term

 

State, in terms of molecular polarity, why 1,2-ethanediol is soluble in water.

Definition

 

It is polar like water

“LIKE DISSOLVES LIKE”

Term

 

When is a gas most ideal?

Definition

 

High Temperature & Low Pressure

(PLIGHT)

Term

 

What happens to the freezing and boiling point when salt is added to water?

Definition

 

F.P. decreases

B.P. increases

Term

 

What is entropy?

What phase has the most entropy?

Definition

 

Disorder of a system.

gas

Term

 

Name 3 ways to increase the rate of a reaction

Definition

 

 Increase temperature

 Increase concentration

 Increase surface Area

Increase pressure(gas)

Add a catalyst

Term

 

Why does increasing the temperature increase the rate of a reaction, in terms of the collision theory?

Definition

 

There are more collisions.

Term

 

How does a catalyst increase the rate of a reaction?

Definition

 

Lowers the activation energy.

Term

 

What happens to the rates and concentration at equilibrium?

Definition

 

Rates are EQUAL

Concentrations are constant.

Term

 

What type of positive ions do acids produce in water?

Definition

 

Acids: Hydrogen(H+) or hydronium.(H3O+)

Term

 

What type of negative ions do bases produce in water?

Definition

 

Bases: Hydroxide (OH-)

Term

 

What is a neutralization reaction?

Definition

 

Acid + Base à Salt + Water

Term

 

What is an electrolyte?

Name three substances that are electrolytes.

Definition

 

Substance that conducts electricity in water.

-Acid, Base, Ionic

Term

 

What occurs during oxidation?

Definition

 

Lose electrons (LEO)

Oxidation number increases

Term

 

What occurs during reduction?

Definition

 

Gain electrons (GER)

Oxidation number decreases

 

Term

 

What is an endothermic reaction?

Draw a potential energy diagram for this reaction.

 

Definition
[image]
Term

 

What is an exothermic reaction?

Draw a potential energy diagram for this reaction

Definition
[image]
Term

 

What is the difference between a voltaic and an electrolytic cell?

Definition

 

Voltaic is spontaneous and converts chemical to electrical energy

 

Electrolytic is non-spontaneous and converts electrical to chemical energy.

 

Term

 

What is the purpose of a salt bridge?

Definition

 

Allow the flow of ions.

Term

 

What is the difference between a saturated and unsaturated hydrocarbon in terms of bonding?

Definition

 

Saturated- all single bonds between C's.

Unsaturated- double or triple bond between two C's.

Term

 

What is an isomer, in terms of structural and molecular formula?

Definition

 

Same Molecular formula, but different structural formula.

Term

 

Identify the type of organic reactions shown.

(a.)  Br2 + CH4 → CH3Br + HBr

(b.) C4H8 + Cl2 → C4H8Cl2

 

Definition

 

(a.) Substitution

     (b. )Addition

 

Term

 

2SO2(g) + O2(g)ßà 2SO3(g) + energy

Explain, in terms of LeChatelier’s principle, why the concentration of SO2(g) increases when the temperature is increased.

 

Definition

 

Shifts left.

Term

 

a. Explain, in terms of attraction, why a substance has a low boiling point.

 

b. Explain, in terms of attraction, why a substance has a high  boiling point.

Definition

 

a. Low= Weak forces.

b. High =Strong forces

Term
[image]
Definition

 

A- Reactants

B- Heat of Reaction

C- Products

D- Activation Energy

Term
Describe how an ionic bond is formed in terms of elements and electrons
Definition

metal and nonmetal.

Electrons are transferred

Term
Describe how a covalent bond is formed in terms of elements and electrons
Definition

nonmetal and nonmetal

electrons are shared

Term
Which way does heat flow?
Definition
From a higher temperature to a lower temperature
Term
Explain why group 18 elements are stable, in terms of atomic structure
Definition
They have complete outer shells
Term
Name 7 organic reactions
Definition
Addition, Substitution, Saponification, Esterification, Combustion, Polymerization, Fermentation
Term
Name 3 types of nuclear reactions
Definition
fission, fusion, and transmutation
Term
How do electrons flow in an electrochemical cell?
Definition
Anode to cathode
Term
Name the 3 homologous series of hydrocarbons
Definition
Alkane, Alkene, and Alkyne
Term
If the pH of a solution changes from 3 to 5, what happens to the hydrogen ion concentration?
Definition
The H+ ion concentration decreases 100x
Term
What element is present in all organic compounds?
Definition
carbon
Term
Compare the number of moles of H+ ions to the number of moles of OH- ions in the titration mixture when the HCl(aq) is exactly neutralized by the NaOH(aq)
Definition
The number of ions is the same
Term
Describe an exothermic reaction
Definition
Energy is released
Term
What 3 quantities are always conserved?
Definition
mass, energy, and charge
Supporting users have an ad free experience!