Science 1A Final Flashcards
ACE THAT FINAL (77 cards)
1
Q
What is the Atomic Mass?
A
An atoms mass in amu with a decimal point.
2
Q
Do protons have mass?
A
Yes, 1amu
3
Q
Do protons have a charge?
A
Yes, a positive charge of 1.
4
Q
What happens when you change the amount of protons?
A
The charge increases by 1, the mass increases by 1amu, and the element changes.
5
Q
Where do protons live?
A
In the nucleus of an atom
6
Q
What is the abbreviation for proton?
A
P+
7
Q
Do neutrons have mass?
A
Yes, 1amu
8
Q
Do neutrons have a charge?
A
No!
9
Q
What happens when you change the amount of Neutrons?
A
The weight increases by 1amu creating and isotope of the same element.
10
Q
Where do neutrons live?
A
The nucleus
11
Q
What is the abbreviation for neutron?
A
N°
12
Q
Do electrons have mass?
A
No! (Technically they have a mass of 0.00055amu but it’s so minuscule it is ignored)
13
Q
Do electrons have charge?
A
Yes, a charge of negative one.
14
Q
What happens when you change the amount of electrons?
A
The charge decreases by one and, depending on the situation, it could add an orbital.
15
Q
Where do electrons live?
A
Orbitals
16
Q
What is the abbreviation for electron?
A
e-
17
Q
What are orbitals?
A
Rings of electrons that surround the nucleus?
18
Q
List the amoung of electrons per orbital
A
2,8,8
19
Q
What is the valence shell?
A
The last orbital around an atom
20
Q
What are valence electrons?
A
The electrons on the valence shell
21
Q
Why is the valence shell and valence electrons important?
A
Because of the Octet rule, ions want to have a full valence shell (8 or 2 electrons) so the amount of valence electrons helps decide how reactive they are, their charge, and what other ions they bond with.
22
Q
What is an Ion?
A
An atom that has lost or gained electrons and therefore has a positive or negative charge.
23
Q
What is the Octet rule?
A
Ions are most stable (least reactive) when their outermost shell of electrons is full.
24
Q
If an ion has less than 4 veilance electrons will it lose or gain electrons?
A
Lose electrons to stabilize! Adopt a positive charge.
25
If an ion has more than 4 veilance electrons will it lose or gain electrons?
Gain electrons to stabilize! Adopt a negative charge.
26
What are the noble gasses?
They are the gasses in row 18 (the farthest to the right on the periodic table) and they naturally have a full veilance shell meaning they don't need to bond or want to band and are not reactive (very stable)
27
Which rows have what charge?
Row 1:+ 1
Row 2: +2
Row 13: +3
SKIP THE TRANSITION METALS
SKIP ROW 14
Row 15: -3
Row 16: -2
Row 17: -1
ROW 18 IS THE NOBLE GASSES
28
What is an Ionic Compound?
It is a charge based bond where the atoms bonded have a combined charge of zero (stable) and they are comprised of a metal and a nonmetal.
29
How do you write/name an Ionic compound?
First the metal and then the nonmetal. You also need to add subscripts to show the amount of an atom and the end of the nonmetal changes to ide.
For instance: Calcium Chloride is CaCl₂
30
What are the polyatomics (with charges)?
Hydroxide- OH charge -1
Nitrate- NO₃ charge -1
Sulfate- SO₄ charge -2
Carbonate- CO₃ charge -2
Phosphate- PO₄ charge -3
Ammonium- NH₄ charge +1
31
What is a Polyatomic ion?
Two or more atoms bonded together as a group that collectively have a charge.
32
What is the only positively charged Polyatomic?
Ammonium, NH₄ charge +1
33
How do you write/ name compounds with polyatomics?
The polyatomic goes last and the compound has to have a combined charge of zero. If there is one polyatomic in the compound, you DO NOT add parentheses but if there is more than one polyatomic in the compound you DO add parentheses around it and then write the subscript outside of the parentheses to show the amount.
Example- NaOH, Sodium Hydroxide
Mg(OH)₂ Magnesium Hydroxide
34
What are the transition metals?
They are metals that can change their charge unlike other elements.
35
How do you write/ name compounds with transition metals?
The metal comes first then in parentheses after the metal its charge is shown in roman numerals then the nonmetal is written. They need a combined charge of zero to bond.
Example- CuO, Copper (II) Oxide but Cu₂O is Copper (I) Oxide. The roman numeral shows the charge of EACH transition metal.
36
What is a Diatomic Gas?
It is an element that exist as pair of atoms when the element is by itself. It's correct to have one diatomic gas when its in a compound.
37
What are the Diatomic Gasses?
HOFBRINCL (7)
H ₂- Hydrogen
O₂ - Oxygen
F₂ - Fluorine
Br₂ -Bromine
I₂ - Iodine
N₂ - Nitrogen
Cl₂ -Chlorine
38
Do the diatomic gasses charge double because there are two when existing alone?
No! It has the same charge as one of that atom.
39
What is the Law of Conservation of Energy?
Energy cannot be destroyed or created, only transferred.
40
What is the Law of Conservation of Matter?
Matter cannot be destroyed or created, only rearranged.
41
What is a mole?
It is a unit of measurement that helps figure out an elements weight in grams because 1 mole of an element is equal to it's atomic mass in grams.
42
What number is a mole?
Avogadro's Number: 6.0022x10^23
43
What is molar mass?
The mass of one mole of atoms or molecules. Molar mass is grams/mole
44
What is the abbreviation for moles?
mol
45
What do you use molar mass for?
To convert between moles and grams. g/mol or mol/g.
46
How do you convert from moles to the amount of molecules/atoms?
Using Avogadro's number to cancel out mol in the factor label method.
47
How do you convert from molecules to atoms?
You multiply the amount of molecules by the amount of atoms in the compound.
48
What is density?
A ratio of mass to volume, Density=mass/volume. It's also an intrinsic property
49
How do you use the FLM to solve for parts in the density equation?
The given extrinsic property (volume or mass) times the density = unknown extrinsic property?
50
What are the units of density?
mL and cm^3 are the same and are used interchangeably!!
Density- g/mL
Volume- mL
Mass- grams
51
What is Kinetic Energy?
The energy that comes from motion.
52
What are the units in the Kinetic Energy equation?
Joules, Kilograms, Meters per second (m/s)
53
What is Gravitational Potential Energy?
Gravitational Potential Energy is energy stored in an object's position.
54
What are the units in the Gravitational Potential Energy equation?
Joules, Kilograms, Meters per second squared (m/s/s) meters.
55
What is the density of water?
1 g/mL
56
What is the specific heat of water?
4.18 j/g x °C
57
Two elemts bond, what is that chemical reaction called?
Synthesis or Combination
58
A bond breaks into two elements, what is that chemical reaction called?
Decomposition
59
A single atom and a compound (of two atoms) switch and the single atom enters the compound and kicks out one of the two atoms in a compound, what is that chemical reaction called?
Single replacement
60
Two compounds bond and the elements in the compounds switch, what is that reaction called?
Double replacement
61
Properties react with O₂ to produce water (H₂O) and carbon dioxide (CO₂), what is that reaction called?
Combustion
62
What are the units in the heat equations?
Heat is in Joules, mass is grams, specific heat is in J/gx*C, change of temperature is in *C
63
In Calorimetry using the law of conservation of energy what can we assume?
We can assume that the mass x specific heat x change of temperature of water is equal to mass x specific heat x change of temperature of the metal.
64
What does equilibrate mean?
Equilibrate is when a cold substance is put in contact with a hot substance and the cold substance will absorb the energy of the hot substance until they are the same temperature.
65
What is the difference between temperature and heat?
Temperature is a way to measure the energy of a substance but heat is used to refer to the amount of energy. So if a teacup is 100* and a bucket is 50* the teacup had a higher temperature but the bucket is hotter because there are more water molecules. Heat is mass based temperature is not.
66
What are ionic bonds?
A bond between a non metal and a metal where they exchange valence electrons to achieve the Octet rule.
67
What are covalent bonds?
A bond between two nonmetals where electrons are shared to achieve the Octet rule. They take lots of energy to break.
68
What is energy density?
It is the amount of energy (kcal) in a gram of a certain substance.
69
What happens to the reactants in a Chemical reaction?
The bonds break and absorb energy.
70
What happens to the product in a Chemical reaction?
New bonds form and they release energy.
71
What is exothermic?
The surroundings of a chemical reaction gains energy (energy is released). That means the reactant absorbed less energy than the product released.
72
What is endothermic?
The surroundings of a chemical reaction cools down (energy is absorbed). That means the product released more energy than the reactant.
73
What are periods on the periodic table?
Rows
74
What are groups on the periodic table?
Columns, they show metals with a similar chemical properties because they all have the same amount of valence electrons
75
Describe the atomic number.
The amount of protons (or electrons if an element is neutral). Its shown on the periodic table. As the atomic number increases, typically so does reactivity.
76
What is the mass number?
The atomic mass of an element rounded to the nearest full number.
77
How do you name covalent bonds?
If there is only one of the first element in the molecule, do not write mono. Besides that, add a numerical prefix to before every name to show amount and change the ending to -ide.
Ex:
CO₂ -> Carbon Dioxide
