Fireworks and Metals/Non-Metals (Review Deck)

Question 1

What are the two pure substances?

Answer 1

Elements - Are substances that cannot be decomposed into a simpler substance (For example Helium, Copper, etc.)

Compounds - Are substances made up of two or more elements combined in fixed proportions

Question 2

What are the two types of mixtures?

Answer 2

Heterogenous - When two or more elements/compounds are combined but not uniformly mixed (If the different ingredients can be seen like pizza, salad, cookies, it is considered heterogenous)

Homogenous - When two or more elements/compounds are combined, but are uniformly mixed (If the ingredients cannot be seen like cola, milk, and air it is homogenous)

Question 3

How does each of the three states affect the molecule interaction?

Answer 3

Solid - Molecules are locked in place, and are not able to move past each other

Liquid - Molecules are not as densely packed, and are able to move past each other

Gas - Molecules are spread out, and move around very fast

Question 4

Atoms are identical no matter the state?

Answer 4

True

Question 5

What is matter

Answer 5

Everything that we touch and feel, and breathe, are matter, which are made of atoms

Question 6

Can atoms have the ability to be broken down physically and chemically?

Answer 6

No atoms are not able to be broken down physically and chemically

Question 7

What are the four components of an atom?

Answer 7

Nucleus - Is a extremely small and dense center of an atom, in which contains both the protons and neutrons

Protons - Are positively charged particles located in the nucleus

Neutrons - Are neutrally charged particles that are located in the nucleus

Electrons - Are negatively charged particles that surround the atom

Question 8

What is the Atomic Number used for?

Answer 8

Scientists use it to show the amount of protons that are in the nucleus of the atom, and also shows the amount of electrons the atom has

Question 9

What is the Mass Number used for?

Answer 9

The mass number is used to show the combined amount of both protons, and neutrons that are in the nucleus

Question 10

What is the formula to find the amount of Neutrons

Answer 10

Mass number - Atomic number

Question 11

What are Isotopes?

Answer 11

Are atoms of the same element, but have a different amount of neutrons and mass number

Question 12

Why can’t electrons be pinpointed?

Answer 12

Electrons travel too fast for the human eye to see

Question 13

What are Energy Levels

Answer 13

Every atom has energy levels that becomes increasingly further away from the nucleus each level, with the energy level closest to the nucleus having lowest energy

Question 14

What are the Purposes of Energy Levels?

Answer 14

Electrons are able to fill out these energy levels

Question 15

How Many Electrons can be Within Each Energy Level?

Answer 15

Energy Level 1: 2 x (1)^2 = 2

Energy Level 2: 2 x (2)^2 = 8

Energy Level 3: 2 x (3)^2 = 18

Energy Level 4: 2 x (4)^2 = 32

Question 16

What is Excitation within Electrons

Answer 16

When Electrons are supplied with energy, they are able to jump from a lower energy level to a higher energy level (Called the transition from ground state to excited state)

Question 17

What are the Three (maybe four) ways an Electron can Receive Energy

Answer 17

1. An electrical current
2. A flame
3. A high energy light source

Another way is through a chemical reaction

Question 18

What Happens After an Electron is Excited?

Answer 18

An electron is only excited momentarily, until it eventually falls back into ground state

Question 19

What Happens When an Electron Goes Back to Ground State

Answer 19

There is a specific amount of energy (photon) that will be emitted which corresponds a specific colored light (called Fluorescence)

Question 20

How Does Amount of Energy Affect Electrons

Answer 20

The more energy an electron is supplied, the farther distance it can jump in the energy levels

Question 21

How does Amount of Energy Affect the Emitted Colors?

Answer 21

The color of light produce depends on how far the electron falls

Electron falling from 2 -> 1 produces low light energy
Electron falling from 5 -> 1 produces higher light energy

Question 22

What are the 3 other Applications of Fluorescence?

Answer 22

1. Counterfeit detection
2. Glow in the dark mini putt
3. Marine fish identification

Question 23

What are the Three Steps on how Fluorescence Work in Glowsticks?

Answer 23

Electrons can also be provided energy by a chemical reaction called chemiluminescence or if exposed to high energy light (UV light)

Step 1: At the moment that the glowstick is cracked, the diphenyl oxalate will come into contact with the hydrogen peroxide, creating a peroxyacid ester

Step 2: When the peroxyacid ester decomposes, energy is released and excites the electrons within the dye compounds

Step 3: The electrons then return back to ground state, and releases the ‘glowing light’

Question 24

How do Fireflies glow?

Answer 24

Fireflies contain D-Firefly Luciferin, which becomes excited and relaxed back to ground state by emitting cold light (hot light kills the firefly)

Question 25

How do Certain Jellyfish Glow?

Answer 25

Jellyfishes contain luciferin, which can be oxidized within the presence of an enzyme called 'luciferase' which causes a chemical reaction that emits a photon of light

Question 26

How is Chemiluminescence used for Blood?

Answer 26

It is a method used at a crime scene in which the iron found within hemoglobin can catalyze a reaction of luminol, which emits blue light for 30 seconds

Question 27

What are the Eight Different Properties of Metals?

Answer 27

1. Solid at room temperature (Mercury being the exception) 2. Conducts heat and electricity 3. Lustrous (Shiny) 4. Malleable 5. Ductile (Made into wire) 6. Hard 7. Dense 8. Possesses high melting and boiling points

Question 28

What are Valence Electrons?

Answer 28

Valence electrons are electrons located on the outermost shell which are able to be removed from the atom easily

Question 29

What is the Valence Electron Trends?

Answer 29

Elements in the same row from left to right: Valence electrons will increase by one Elements in the same column: Valence electrons stay the same Remember that He only has 2 valence electrons

Question 30

What is the Octet rule?

Answer 30

The octet rule states that the outermost shell must be full to achieve stability

Question 31

What is Ionic Bonding?

Answer 31

An ionic bond is an electrostatic attraction between both an metal (cation), and an nonmetal (anion), which involves in an exchange of electrons

Question 32

How do Cations and Anions Work Together?

Answer 32

Cations (metals) are positively charged atoms that are generated due to a loss in electrons Anions (nonmetals) are a negatively charged atoms that are generated due to a gain in electrons Both need each other in order to achieve a stable octet

Question 33

How are Ionic compounds named?

Answer 33

Metal + nonmetal + 'ide'

Question 34

What are Metallic Crystals?

Answer 34

Has a shape that is similar to an ionic crystal, however all atoms are positive, which means there is no positive-negative reaction

Question 35

How do Atoms in a Metallic Crystal Stay Together?

Answer 35

The Electron Sea Model shows the nuclei of metals are surrounded by a sea of delocalized electrons which are able to be distributed and moved across any atoms, which holds the entire crystal together

Question 36

What is the Conductivity within the Electron Sea Model?

Answer 36

When energy is supplied to one end of the metal, the electrons from the current will hop through the electron sea and passes to the other end An example of this is copper wires

Question 37

What is the Shininess Within the Electron Sea Model?

Answer 37

Electrons are able to absorb any incoming light, and will re-emit the light which causes the metal to shine

Question 38

What is the Malleability and Ductility of the Electron Sea Model?

Answer 38

The ionic crystal has delocalized electrons which helps keep the metallic lattice stable, as atoms move over each other, the electrons will move as well to keep the structure stable

Question 39

Why are Ionic Crystals not Malleable?

Answer 39

If an ionic crystal were to be hit by a hammer, it would shatter because the atoms would slide past each other causing like charges to be next to each other, causing a strong repulsion, resulting in the crystal shattering

Question 40

What is the Melting/Boiling Point in the Electron Sea Model

Answer 40

The attraction between the metal cations and the delocalized electrons are very high because they want to stay together, as delocalized electrons increases, the hardness, and boiling point also increases

Question 41

What is Specific Heat Capacity?

Answer 41

A measurement of how much heat energy must be absorbed before it changes temperature

Question 42

What are the Steps to Find the Specific Heat Capacity?

Answer 42

The Specific Heat Capacity can be found by using a technique called 'calorimetry' 1. A cube is first placed in a Styrofoam cup filled with a known amount of water at a known temperature 2. Assuming the cup is insulated, whatever heat is gained/lost by the metal is then absorbed/withdrawn by the water

Question 43

What are the Six Properties of Nonmetals

Answer 43

1. Most are gaseous at room temp 2. Are poor conductors for both heat and electricity 3. Are dull and colorless 4. Are brittle 5. Low density 6. Has a low melting point

Question 44

What is the Reaction Between two Nonmetals Called?

Answer 44

The moment two nonmetals come into contact, the valence electrons are shared to create a stable octet calling a 'covalent bond'

Question 45

How are Covalent Compounds Named?

Answer 45

Same as ionic compounds except a prefix must be added for both nonmetals prefix + nonmetal + nonmetal + ide Prefixes would be: 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca

Question 46

What is Covalent Bonding?

Answer 46

Is when electrons are not shared equally, and instead is depended on the electronegativities of both atoms

Question 47

What is Electronegativity?

Answer 47

The ability in which can atom can attract bonding electrons

Question 48

What are all the Bond Types and Their Electronegativies?

Answer 48

Non-polar covalent: Equal sharing of electrons which has a electronegativity difference of < 0.4 Polar Covalent: Unequal sharing of electrons which has an electronegativity difference of between 0.4 and 1.8 Ionic Bonding: An ionic bond is formed due to the large electronegativity difference which is > 1.8

Question 49

What is the Difference Between Covalent and Ionic Bonding?

Answer 49

Covalent bonding: Is when valence electrons are shared between atoms and exists as molecular units Ionic Bonding: Is when valence electrons are transferred between each other and exists as a ordered array

Question 50

What are the Five Properties of Metalloids?

Answer 50

1. Are intermediates between metal and non-metals 2. Most are solid at room temperature 3. Some are able to conduct heat and electricity, like silicon and germanium 4. Some are lustrous 5. Tends to be brittle

Question 51

Liquids are compressible and have a fixed volume| True or false?

Answer 51

False

Question 52

Solids are incompressible and have a fixed volume True or false?

Answer 52

True

Question 53

Gases are compressible and have variable shape and volume| True or false?

Answer 53

True