Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

10 Science > Chemistry > Flashcards

Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
Biology 101 flashcards
1
Q

What are atoms?

A

The smallest particle of a chemical element.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the periodic table?

A

The arrangement of all known elements in order of atomic number.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are groups in the periodic table?

A
  • Groups refer to the vertical columns in the periodic table.
  • Group number = the number of valence electrons.
  • elements in the same group share similar properties.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are periods in the periodic table.

A
  • Periods refer to the horizontal rows in the periodic table.
  • Period number = the number of electron shells.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Describe metals, non-metals, and metalloids.

A
  • Metals are elements that tend to lose electrons (found on left side of the periodic table).
  • Non-metals are elements that tend to gain electrons (found on right side of the periodic table.
  • Metalloids are elements with properties of both metals and non-metals.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Describe electronegativity.

A
  • An atoms ability to gain electrons.
  • higher electronegativity = more likely to gain electrons.
  • increases across a period.
  • decreases down a group.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Describe electron shells.

A
  • Different energy levels within the atom that hold electrons
  • closer to the nucleus = lower energy
  • further from the nucleus = higher energy.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Describe ionic bonding.

A
  • Ionic compounds formed from the transfer of electrons between a metal and a non-metal
  • Ions are charged atoms that have lost or gained electrons
  • Ionic bond is an electrostatic connection between a positive and negative ion.
  • Cations - positively charged (lost electrons)
  • Anions - negatively charged (gained electrons)
  • High electronegativity (non-metals) will gain electrons
  • Low electronegativity (metals) will lose electrons
  • Swap and drop
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Describe covalent bonding.

A
  • Molecules formed between a non-metal and a non-metal as a result of sharing electrons.
  • shared electrons are attracted to the positive nuclei.
  • not as strong as ionic bonds.
  • Single bond - each atom shares one electron (2)
  • Double - each atom shares two electrons (4)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Describe the characteristics of an electron dot diagram and structural diagram.

A
  • Used to illustrate covalent bonds
  • Electron dot diagram includes all valence electrons.
  • Structural diagrams only show covalent bonds.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Describe chemical reaction.

A
  • Atoms are rearranged, substances break bonds to form new bonds, producing a new substance.
  • Indicators:
  • colour change
  • gas production
  • form precipitate (solid)
  • energy is produced or absorbed (heat/sound/light)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Word equations.

A
  • Describe chemical reactions by writing full name of reactants and products.
  • E.g. Hydrochloric acid + sodium hydroxide –> sodium chloride + water.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Law of conservation of mass.

A
  • Matter cannot be created or destroyed, only changed in form.
  • Number/type of atoms must be balanced for reactants and products.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Chemical equations.

A
  • Use formula to show how atoms in reactants rearrange to form products.
  • E.g. HCl(aq) + NaOH(aq) –> NaCl(aq) + H20(l)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Exothermic and Endothermic reactions.

A
  • Exothermic reactions:
  • Release energy into surroundings
  • Release heat/light/sound
  • less energy in products than reactants.
  • Endothermic reactions:
  • Absorb energy from the surroundings
  • Cold surroundings / cold test tube
  • More energy in products than reactants.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Decomposition reaction.

A
  • a single compound breaks down into two or more elements.
  • AB –> A + B
  • CuCO3(s) –> CO2(g) + CuO(s)
16
Q

Synthesis reaction.

A
  • two or more reactants combine to form one product.
  • A + B –> AB
  • 2H2(g) + O2(g) –> 2H20(l)
17
Q

Single displacement reaction.

A
  • an element reacts with a compound, replacing one element within that compound.
  • A + BC –> AC + B
  • Fe(s) + CuSO4(aq) –> Cu(s) FeSO4(aq)
18
Q

Double displacement reaction.

A
  • two compounds react, the positive cations and negative anions in the two reactants switch places, forming two new substances.
  • AC + BD –> AD + BC
  • CuSO4(aq) + 2NaOH(aq) –> Cu(OH)2(s) + Na2SO4(aq)
19
Q

Precipitation reaction.

A
  • a type of double displacement reaction
  • soluble aqueas solutions react to form an insoluble solid.
  • 2KI(aq) + Pb(NO3)2(aq) –> PbI2(s) + 2KNO3(aq)
20
Q

Combustion reaction.

A
  • Hydrocarbon reacts in the presence of oxygen to produce carbon dioxide and water vapour (and heat)
  • Hydrocarbon + Oxygen –> Carbon dioxide + Water
  • CH4(g) + 202(g) –> CO2(g) +2H20(g)
21
Q

Neutralisation reaction.

A
  • An acid and a base react to produce water and a salt
  • Acid + Base –> Water + Salt
  • H2SO4(aq) –> 2NaOH(aq) –> 2H2O(l) + Na2SO4(aq)
22
Q

Collision theory.

A
  • For a chemical reaction to occur:
  • particles must collide
  • with proper orientation
  • colliding with enough energy to meet minimum activation energy.
23
Q

Activation energy.

A

The minimum amount of energy required at which a collision will turn reactants into products.

24
Q

Rate of reaction.

A
  • Chemical reactions occur at different rates.
  • Rate of reaction refers to the speed at which a chemical reaction proceeds.
25
Q

Describe how agitation affects rate of reaction.

A
  • As a chemical reaction progresses the reactant particles are used up.
  • The fewer reactant particles = the fewer collisions occur causing the reaction rate to slow.
  • Agitation increases particle moment, causing collisions to occur more frequently, increasing the rate of reaction.
26
Q

Describe how surface area affects rate of reaction.

A
  • In solid reactants only particles exposed at the surface can react.
  • Smaller particles have a larger surface area than larger particles, exposing more of the substance to reactants.
  • Increasing surface area increases frequency of collisions, increasing rate of reaction.
27
Q

Describe how temperature affects rate of reaction.

A
  • Increasing temperature increases kinetic energy of particles causing particles to move faster.
  • The faster particles move, the more frequently collisions will occur, increasing the rate of reaction.
28
Q

Describe how concentration affects rate of reaction.

A
  • Concentration refers to the number of particles present in a particular volume.
  • Increasing the concentration of reactant particles increases the frequency of collisions, resulting in an increased rate of reaction.
29
Q

Describe how catalysts affects rate of reaction.

A
  • A catalyst is a chemical that speeds up a chemical reaction without being consumed.
  • Catalysts increase the rate of reaction by temporarily binding to reactants, providing proper orientation for a successful collision to occur.
  • or provide an alternative reaction pathway with lower activation energy, increasing the number of successful collisions.
  • Increasing the number of successful collisions increases the rate of reaction.

10 Science (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions