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Chem 20 > *Review* > Flashcards

*Review* Flashcards

Review of Chem 10

1
Q

Matter is everything with?

A

Mass and Volume.

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2
Q

Matter separates into which two categories?

A

Pure substances, and mixtures.

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3
Q

What number is close to the amount of the naturally occurring elements?

A

90

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4
Q

How many synthetic elements are there?

A

25

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5
Q

What are the main characteristics of metals?

A
  1. Good at conducting electricity and heat.

2. Are malleable and ductile.

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6
Q

What are the characteristics of non-metals?

A
  1. They do not conduct heat and electricity.

2. They are not malleable or ductile.

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7
Q

What are the characteristics of metaloids?

A

They have characteristics that fit in-between metals and non-metals.

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8
Q

What does ductile mean?

A

It means to be put in a cylindrical wire shape.

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9
Q

Pure substances are separated into?

A

Elements and compounds.

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10
Q

Mixtures are separated into?

A

Homogeneous (looks like one thing): “solutions” and heterogeneous (looks like several things): “suspensions and colloids”

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11
Q

What are alkali metals

A

They are group 1, the farthest left group (not including hydrogen).

They are super reactive and soft.

Only have one electron in valance shell

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12
Q

What are alkali earth metals?

A

They are the second group, with two valence electrons

They are like alkali metals except less reactive and soft.

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13
Q

What are Nobel gases?

A

They are group 18 and are not reactive because they are stable.

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14
Q

What are halogens?

A

Group 17 and are the most reactive non-metals.

They need one electron to become stable.

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15
Q

What are periods and how many are there?

A

They are the 7 rows on the periodic table

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16
Q

What are groups and how many are there?

A

They are the 18 columns in the periodic table

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17
Q

What are atoms?

A

They are the smallest particle of an element that can undergo a chemical reaction.

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18
Q

What are atoms made up of?

A

Subatomic particles (protons, electrons, and neutrons)

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19
Q

What are protons (p+)?

A

p+ are +1 charge

they have an atomic mass of 1

and they live in the nucleus

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20
Q

What is an electron (e-)?

A

e- has a charge of -1

Has 1/1836 mass of a proton

Orbits the nucleus

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21
Q

What is a neutron (n°)?

A

n° has a mass of 1

Zero charge

And lives in the nucleus

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22
Q

What does the atomic number represent?

A

Number of protons.

23
Q

What does the atomic mass represent?

A

A total number of protons and neutrons.

24
Q

What are the energy levels?

What is the valence shell?

A

Energy levels are the things that hold electrons.

Each level can hold a certain amount of electrons

It goes 2,8,8,8 (first level to 4th level)

The valence shell is the outermost shell that did or does have electrons.

25
Q

What are isotopes?

A

Same element different amount of neutrons.

All isotopes are radioactive.

The average amount (in the environment) and average mass of isotopes (plus the element) make the atomic number.

All isotopes are radioactive.

26
Q

When does an atom become stable?

A

When it has a full valence shell.

27
Q

What is an ion?

A

It is when atoms lose or gain electrons to become stable. (Like Nobel gases)

This is called the duplet (2 electrons or energy level one), octate rule (8 the rest of the energy levels).

This makes the ion positively (loses electrons) or negatively (gains elections) charg ed.

28
Q

How do you name ionic compounds?

A

Cation, anion-ide

Example: sodium and fluorine = sodium fluoride

(Must be in lowercase letters)

29
Q

How to create ionic compounds

A

Ionic compounds must have zero charge.

You take two atoms make then a cation and a anion and you put them together in the lowest ratio to become stable.

30
Q

What is a cation?

A

It is a positive ion (fewer electrons than normal).

31
Q

What is a anion

A

A negatively charged ion (more electrons than usual)

32
Q

What is a polyatomic ion?

A

Is a group of atoms covalently bonded to create a unit with a charge.

These replace a cation or an anion in an ionic compound. (Usually a caution)

Do not use prefix -ide when putting them in ionic compounds.

Ex: NH4, OH,

33
Q

Which charge do you use for ions?

A

Always use the MOST COMMON one unless instructed otherwise.

34
Q

What are molecular compounds?

A

They share electrons to complete their outer shell to become stable.

Always non-metals.

They do this to make fulfill the duplet or octate rule.

35
Q

What are molecular elements?

A

Molecules with only one kind of atom.

These are both diatomic and polyatomic elements.

36
Q

What are Diatonic elements?

A

Elements that exist in the world as groups of two

These include:

H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l) I2(s)

37
Q

What are Polyatomic elements?

A

Same as diatonic but it is more then 2.

O3(g) P4(s) S8(s)

38
Q

What are the prefixes for molecular compounds?

A

(Based on how many atoms and that there is no hydrogen involved)

Do not use mono for the first atom and use -ide at the end.

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

Ex. Tetraphosphorus decaoxide (P4 + O10)

39
Q

Molecules with hydrogen which has names you need to remember

A

Check chart!!!

40
Q

How to names acids ( IUPAC name)?

A

You put aqueous + molecule or element name + acid

In acids, you balance charges like ionic compounds (with hydrogen being cation) even though there molecular.

41
Q

Properties of bases?

A

Ionic compounds with a cation and a hydroxide (OH)

42
Q

S8 is?

A

Sulfur molecule (same with all other molecular elements).

43
Q

Acids that need to be memorize

A

Sulfuric acid = H2SO4
Hydrochloric acid = HCl
Nitric acid = HNO3

44
Q

How to name just an ion?

A

Metals = name + ion

Non-metals = name-ide + ion

45
Q

What are the Solubility properties of ionic compounds?

A

They are solid at room temp.

High boiling and melting points

When they’re put in water and are highly soluble in water their states become aqueous (aq).

Compounds Less soluble in the water stay solid (s).

(Use a solubility chart to find if an ionic compound is soluble)

46
Q

What are formation reactions?

A

Element + element = compound

A + B = AB

(Remember states)

47
Q

What are the Three different types of ways to display reactions?

A

Word equation: sulphur + oxygen = sulfur dioxide

Skeleton equation: S8 + O2 = SO2

Balanced equation: S8 + 8 O2 = 8 SO2

(Remember states for both skeleton and balanced equation)

48
Q

What is a decomposition reaction

A

Compound = element + element

BA = B + A

(Remember states )

49
Q

What is a decomposition reaction

A

Compound = element + element

BA = B + A

(Remember states)

50
Q

What is a hydrocarbon combustion reaction?

A

Cx + Hy + O2 = CO2 + H2O

(Where x and y are variables)

(Remember states)

(Water is always a gas in these reactions)

51
Q

What is the alkane formula?

A

CxH(2x+2) ( always ends in -ane)

CH4 = methane

C2H6 = ethane

C3H8 = propane

C4H10 = butane

(Continues as liquids instead of gases, and with molecular naming prefixes)

C5H12 = pentane

52
Q

What are Single replacement reactions?

A

A(Metal/Non-metal) + BC = B + AC

or C + BA (depending if it is a metal or not)

(Remember states)

53
Q

What is double replacement reaction?

A

AB + CD = AD + BD

Remember states

Chem 20 (6 decks)

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