Chem 10 vocab Flashcards
(57 cards)
1
Q
Alkali metals
A
- group 1
- soft, shiny and silver
- very reactive with water
- reactivity increases as you move down the group
- their compounds are soluble in water
2
Q
Alkaline Earth Metals
A
- group 2
- shiny, silver, but not as soft as group 1
- form oxide coatings when exposed to air
- coumpounds are white, but less soluble than group 1
3
Q
anion (-)
A
- formed when non-metals gain electrons
- negatively charged
- charge = number of electrons that are gained (- = 1 was gained)
- change to “ide” (chlorine atom -> chloride ion)
4
Q
Atom
A
smallest part of an element with properties of an element.
5
Q
atomic number
A
number of protons and electrons
6
Q
Bohr Model
A
Each energy level has a max number of electrons that can reside in it, and they can jump from one level to another. Electrons travel in seperate orbits and are attracted to the nucleus.
7
Q
cation (+)
A
- formed when metal atoms lose electrons
- positively charged
- charge = the number of electrons that were lost (+ = 1 lost)
8
Q
chemical change
A
a change that is permanent (evidence of gas, precipitate, heat, light)
9
Q
compound
A
A combination of two or more elements
10
Q
Dalton model
A
stated that all matter is composed of atoms that can’t be created or destroyed into smaller particles. All atoms of an element are identicle.
11
Q
Element
A
Made of atoms and cannot be broken
12
Q
energy level
A
region of space where electrons are found
13
Q
group
A
- columns
- number of electrons on outermost layer (valence) = group number
14
Q
Halogens
A
- group 17
- elements are poisonous
- react with alakali metals to form salt
- reactivirty increases as you move up the group
15
Q
heterogeneous mixture (mechanical mixture)
A
A mixture where you can see the parts
16
Q
homogeneous mixture
A
a unifrom mixture, usually a liquid (iced tea, chocolate milk)
17
Q
ion
A
- electricaly charged atom or group of atoms
- do not have an equal amount of protons and electrons
- more protons = positive charge
- more electrons = negative charge
18
Q
ionic compound properties
A
- have high melting points
- retain crystal shapes (lattice)
- are soluble in water
- are conductors - are electrolytes
19
Q
isotope
A
atom of an element with a different number of neutrons from protons
20
Q
mass number
A
number of protons + number of neutrons
21
Q
metalloids
A
- solids and gasses
- between non-metals and metals
- some can conduct
22
Q
Metals
A
- most are shiny and grey
- malleable and ductile
- conducts
- solids at room temperature (except mercury)
- forms cations (+ ions)
- on left side of staircase
23
Q
mixture
A
two or more substances combined
24
Q
molecular compound properties
A
- low melting points
- crumble easily (don’t maintain crystal lattice)
- most are not soluble in water
- low or no conductivity - not an electrolyte
25
Noble gases
* **group 18**
* are unreactive
26
non-metals
* can be L, S, or G at room temp
* some highly reactive and some unreactive
* form anions (- ions)
* right side of staircase
* vary in color and dull
* poor conductors
* not malleable, and are brittle
27
number of neutrons can be calculated...
mass number - number of protons
28
octet rule
atoms gain or lose electrons to have a full valence shell.
* a transfer of electrons occur from the **metal to the non-metal**
29
Period
* rows
* the number of energy levels occupied by electrons = period number
30
physical change
a change in form that is reversable (H2O melting to freezing)
31
Pure Substance
It has one type of particle (anything on periodic table)
32
Quantum Mechanical model
* today's model of the atom
* Electrons exist in the cloud of negative that surrounds the nucleus
* nucleus contains the protons (+) and neutrons (0)
33
Rutherford Model
Hypothesized that the atom is mainly empty space but each atom has a small positively charged core (nucleus). Nucleus accounts for majourity of the atom's mass.
34
suspension
a heterogeneous mixture that settles
35
Thompson Model
Accounted for the existence if small negative charges, and these electrons have shells or energy levels.
36
transition metals
these elements have a wide range of chemical and physical properties.
37
water polarity
one end is negative and the other is positive.
* has a higher boiling point because of its polarity
* negative oxygen and one positive hydrogen
38
acid
coumpoud that dissolves in water to form a solution with a **pH less than 7**
39
base
a compound that dissolves to form a solution with **a pH greater than 7**
40
buffer
a substance that can keep a pH constant, even if an acid or base is added
41
Acid properties
* sour
* not slippery
* corrodes metal
* litmus turns red
* conducts
* under 7 pH
42
base properties
* bitter
* slippery
* doesn't corrode metal
* litmus turns blue
* conducts
* over 7 pH
43
neutralization
* when acids and bases react together, both acid and basic properties dissapear
* this reaction produces water and salt
44
chemical reaction
* formation of a gas
* formation of precipitate
* color change
* energy change (heat, light, electricity)
45
Endothermic
reactions that **absorb** energy
46
exothermic
reactions that **release** energy
47
enzyme
chemicals that speed up a reaction but are not used up by it
48
law of conservation of mass
the totoal mass of all the reactants is equal to the total mass of all the products
49
formation reaction
two element combine to form a compound
A + B = AB
50
decomposition reactions
breaking a product down into it's reactants (opposite of formation reaction)
AB = A + B
51
(hydrocarbon) Combustion
CxHy + O2 = CO2 + H20
(usually burning)
52
single replacement reaction
a reactive compound reacts with an element
A + BC = B + AC
non-metals trade places
53
double replacement reaction
2 ionic compounds react (ususally occur in solutions)
AB + CD = AD + CB
54
find mass
m = nxM
55
find molar mass
M = m/n
56
find moles
n = m/M
57
covalent bonds
when atoms **share** electrons
* this happens in order to fill the valence shell (full octet)
