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Chem 101 > EXAM TWO STUDY CARDS > Flashcards

EXAM TWO STUDY CARDS Flashcards

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1
Q

Is Light a state of matter?

A

No, Light is a form of electromagnetic radiation

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2
Q

Is Light a form of radiation?

A

Yes, Light is a form of electromagnetic radiation

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3
Q

What is the order for Light, least to most energtic?

A

ROYGBIV, Red the least Violet the most

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4
Q

Why do we perceive light?

A

Excited CORE electrons in atoms make large “jumps” when exposed to energy, and those jumps produce a light according to the distance jumped when they return to a relaxed state

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5
Q

What is Atomic Radius?

A

The distance between Nucleus and Valence Electrons

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6
Q

As you go down a period, Atomic Radius…

A

increased. Adding more protons and neutrons makes the atom larger. Think adding coat layers in the winter.

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7
Q

As you go across a period, Atomic Radius…

A

Decreases, because the electrons are bound tighter and tighter the more there are. Think adding more and more magnetic force= tighter packed.

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8
Q

What is Ionization Energy?

A

Quantity of energy required to move an atom from a neutral form to a positive cation (By taking an electron from it.) Think Ion-ization, cat-ion, paws-itive.

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9
Q

As you go down a period, Ionization Energy…

A

Decreases. The more electrons you add, the more the radius is increased. As the electrons are farther away from the nucleus, they will be more easily pulled away.

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10
Q

As you go across a period, Ionization Energy….

A

Increases. The radius decreases, and therefore the nucleus’s grip on the electrons is a lot stronger, meaning you need more energy to yank away an electron.

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11
Q

What is the Heisenberg Uncertainty Principle?

A

You can predict the position or the velocity of an electron, not both.

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12
Q

List the 4 Quantum Model Orbitals, and how many electrons they can hold, and which periods they correspond to

A

S can hold 2, Groups 1a and 2A
P can hold 6, groupo 3a to 8 a,
D can hold 10, Transition metals
F can hold 14, Inner Transition metals

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13
Q

Pick an Element. Write it’s longform Electron Configuartion

A

Look it up n see if ur correct

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14
Q

Pick an element. Write it’s short form Electron Configuration.

A

Look it up. It should start with the nearest Noble Gas.

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15
Q

Take an electron configuartion. pick out the valence electrons

A

It should be the largest obital. IE 3d104p6, even though p is less valence, it’s got the larger orbtial, 4 to 3, so this one would be 6 valence.

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16
Q

What does the Law of Constant Composition state?

A

Compounds always contain a fixed proportion of their constituent elements.

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17
Q

What is an Ionic Bond?

A

A Bond between a non-metal and a metal atom. The metal Cation transfers it’s electrons to the Nonmetal Anion, both have full valence shells of 8. Extremely stable compounds as a result. Poor conductors, high melting points, crystalline, dissolve in water.

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18
Q

What is a Covalent/Molecular bond?

A

A bond between two non-metals. The elements will share their valence electrons (co-valence). Soft, poor conductors, lowmelting point, insoluable in water.

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19
Q

What is a metallic Bond?

A

Pretty easy :p a bond between two metals. Good conductor of electricity, variable melting point, hard.

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20
Q

What type of bonds make Diamonds?

A

Covalent: Carbon bonds with Carbon to make Diamonds, making it a covalent bond.

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21
Q

What is a Polyatomic Ion?

A

An ion with two or more atoms (it’s in the name!)

22
Q

Pick a non-transition metal, and give it’s ion.

A

Look up if ur right.

23
Q

What’s strange about Transition metals and Ions?

A

Most Transition metals hold several different ions. Remember Swap and Drop for these guys.

24
Q

Name the 10 prefixes for Covalent Compound namings

A 
1- mono
2-di
3-tri
4-tetra
5-penta
6-hexa
7-hepta
8-octa
9-nona
10-deca
25
Q

What is the suffix for almost all Ionic compounds?

A

-ide.

26
Q

What is the convention for naming Covalent Compounds?

A

Use the quantity prefix for each element unless the first element is solo (PCl3 is Phosphorus Trichloride, P2Cl3 is DiPhosphorus trichloride.)

27
Q

What’s the naming covnention for Hydrated compounds?

A

The noraml names, + (prefix) hydrate. Written as * (number) h20

28
Q

What are the rules for Semimetal compounds?

A

Metal and semimetal, use ionic rules, semi metal and nonmetal, use covalent rules.

29
Q

All Compounds are electrically neutral, true or false

A

True! Use this to hint at Swap n Drop!

30
Q

Try to form a Ionic compound

A

Google it and make sure u got it right

31
Q

Try to form an ionic compound with a transition metal

A

Google it and make sure u wrote it right

32
Q

Try to form a covalent compound

A

google it and make sure u wrote it right

33
Q

What is Electronegativity?

A

The abillity of an atom to draw an electron to itself.

34
Q

Electronegativity’s trend on the periodic table?

A

Top right most electronegative, bottom left least.

35
Q

What are the steps to draw Lewis Dot structure?

A
  1. Count of the available Valence Electrons
  2. Draw the central atom, connect all non-central atoms with two-electron bonds
  3. Satisfy all outer atoms with remaining Valence electrons.
  4. Satisfy inner atoms and distribute remaining electrons
36
Q

If the electronegativity between two atoms is greater than two, the bond is…

A

Ionic. Think, nonmetals are on the right, metals on the left.

37
Q

If the electronegativity is between 2 and 1, the bond created is…

A

Polar Covalent. Think about Transition metals being wonky

38
Q

If the electronegativty difference between 2 atoms is less than 1, the bond is

A

Pure covalent. Think metal bonds and covalent nonmetal bonds.

39
Q

What are special about Hydrogen and Boron in regards to Lewis Dot structures?

A

Hydrogen only needs 2 atoms to be happy, Boron only needs six.

40
Q

When is a molecular Polar?

A

When the electrons are unevenly distributed (note: not bonds, un-bonded electrons.)

41
Q

“Like-dissolves-like” means..

A

Polar susbstances dissolve polar substances, non-polar dissolves non-polar.

42
Q

Polar atoms are often unstable because…

A

Unbonded electrons are very unstable.

43
Q

What is an IMF? List the main three.

A

Inter-molecular force. Dispersion, Dipole-Dipole, Hydrogen are the 3

44
Q

Why do phase changes happen?

A

IMFs are overcome. Solids are where IMFs are at their strongest, gas is the absolute lack of IMFs.

45
Q

How do you tell what IMF is active in any given molecule?

A

Hydrogen bonds form between Hydrogen and N O or F. Dipole-Dipole occurs in any Polar molecules. Disperson occurs in the rest.

46
Q

List IMF and intermolecular forces, strongest to weakest

A

Ionic, Covalent, LARGE jump, Hydrogen Bond, Dipole-Dipole, Dispersion.

47
Q

When faced with two molecules with the same IMF, how do you tell which is stronger and therefore has the higher melting point?

A

Molar mass (mass numbers)

48
Q

What is Surface Tension?

A

The resistance of liquids to spreading their surface area.

49
Q

What is viscosity?

A

The resistance of a liquid to flow.

50
Q

Emulsifiers are..?

A

Things that allow polar substances to mix with nonpolar substances

51
Q

Surfactants are..?

A

Substances that reduce surface tensions.

Chem 101 (3 decks)

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