Chemi Flashcards
1
Q
Chemistry
A
the study of the properties of matter and the changes it undergoes
2
Q
Matter
A
anything that takes up space and has a mass
3
Q
Mass
A
measure of matter that an object contains
4
Q
substance
A
matter that has a definite or constant composition and distinct properties
5
Q
mixture
A
a combination of two or more substances in which the substances retain their distinct identities
6
Q
Compound
A
a substance combined of two or more elements
7
Q
Element
A
A substance that cannot be separated into simpler substances by chemical means
8
Q
homogeneous mixture
A
a uniformed mixture
9
Q
heterogeneous
A
not a uniformed mixture
10
Q
solvent
A
dissolves the solute
11
Q
Solute
A
added to the solvent
12
Q
solution
A
homogeneous mixture consisting of a solvent and solute
13
Q
atomic number
A
protons
14
Q
mass
A
protons and neutrons
15
Q
Freezing water
A
0 C and 32 F
16
Q
Normal Body temp
A
37 C and 98.6 F
17
Q
Boiling water
A
100 C and 212 F
18
Q
celsius to fahrenheit
A
F = °C × (9/5) + 32
19
Q
F to C
A
°C = 5/9(°F – 32).
20
Q
Ions
A
when an atom is electrically charged. When an ion is in a ionic state it will lose or gain electrons.
21
Q
Cation
A
Positive charged
Gains protons looses electrons
22
Q
Anion
A
Negative charge
Loses protons gains electrons
23
Q
Isotope
A
atoms of the same element with different mass numbers
24
Q
chemical change
A
original substance is transformed into a new substance with different properties
example: burning of wood and then the wood turning into ashes
25
Physical change
transformation that does not produce a new substance
Example: Cutting fruit
26
Mole
Amount of substance that contains 6.02*10^23 particles
27
mixtures
consist of 2 or more substances that our Not chemically bonded
28
Homogenous mixture
Uniformly distributed
29
Heterogenous
mixture not uniformly distributed
example: Pizza, Rock, Vegtable soup
30
Solvent
Dissolves the solute
31
Solute
added to the solvent
32
Solution
homogenous mixture consisting of solvent and solute
33
Periodic table
Arranged in groups and periods
Group number shows how many electrons are in a shell
Groups ( Up and Down) Vertical
Periods ( left to right) horizontal
Heavy metals are at the bottom, lighter metals are at the top
34
Alkali Metals
Far left of periodic table
lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr)
35
Alkaline
Left of periodic table
beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
36
Transition metals
Middle of periodic table
Scandium (Sc), yttrium (Y), lutetium (Lu), lawrencium (Lr), titanium (Ti), zirconium (Zr), hafnium (Hf), rutherfordium (Rf), vanadium (V), niobium (Nb), tantalum (Ta), dubnium (Db), chromium (Cr), molybdenum (Mo), tungsten (W), seaborgium (Sg), manganese (Mn), technetium (Tc), rhenium (Re), bohrium (Bh), iron (Fe), ...
37
Metalloid
Right side of periodic table
antimony (Sb), germanium (Ge), silicon (Si), arsenic (As), tellurium (Te), polonium (Po), boron (B), and astatine (At).
38
Halogens
fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At), and tennessine (Ts).
39
Noble gases
Far right
helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), radon (Rn), and oganesson (Og).
40
stioichiometry
part of chemistry that deals with the quantities and numeric relationships of the particles in a chemical reaction
AB+CD>>>>>>ABCD
recant products
41
oxidation and reduction
oxidation and reduction reactions are called redox it involves the transfer of electrons from one element to another
OIL ( oxidation is lost)
RIG ( reduction is gained)
42
oxidation of any element is what?
zero in its natural state there are a few exceptions hydrogen, oxygen, bromine, nitrogen, fluorine
43
Acids (+)
Corrosive to metals
Hydrogen donors
44
Base (-)
Denatures proteins
Hydrogen receptors
45
alpha waves
the emission of the helium nuclei: pass thru paper and skin
46
Beta waves
A product of the decomposition of a neutron. Can pass thru aluminum
47
Gamma Wave
High energy electromagnetic radiation similar to x-rays but more energy. Very penetrating. Can go through 7 feet of concrete and lead.
48
What are the 4 macronutrients
Carbohydrates, Lipids (COOH), Nucleic Acids, Protien
49
Mono
1
50
saccharide
sugar
51
Di
2
52
Oligo
3-6
53
poly
many
54
covalent bond
formed when two atoms share electrons, generally in pairs
ex. H2O
55
Ionic Bond
an electrostatic attraction between two opposite charged ions or cation, anions generally formed between a nonmetal and a metal
example: Na+Cl>>>>NaCl
56
intermolecular forces types
hydrogen bonds, dipole-dipole, dispersion
57
Hydrogen bonds
attraction for a hydrogen atom by high electronegativity elements. Involves fluoride, oxygen and nitrogen
example: H2O, NH3, CHCl3
58
Dipole-Dipole
the attraction of diploid one molecule for the diploid of another molecule. When electrons are shared unevenly
Salt
Polar compound
ionic compound
59
dispersion
when the. electrons concentrate themselves on one side of an atom which causes a momentarily temporary dipole
example: Use of carbon and hydrogen
60
5 types of chemical reactions
Synthesis, single replacement, decomposition, combustion, double replacement
61
Synthesis
two events combine to form a product
two compounds form to make a single product
A+B>>AB
62
Decomposition
Breakdown of a compound into components parts
AB>>A+B
63
Combustion
chemical reactions ( burning of gases). Always contains CO2 and H20
64
single replacement
Consists of more than one active metal reaction with ionic compounds. One element starts out by itself and ends up kicking another element out.
A+BC>>>B+AC
65
Double replacement
reactions that involves two ionic compounds. the positive involve two ionic compounds. The positive and negative ions in two compounds switch places.
AgNO3+KCl>>>AgCl+KNO3
66
how to find mass given density and volume
multiply
67
To find density it’s
mass/volume
68
To find volume you?
Divide mass/ density
69
what is a catalyst
a substance that increases the rate of a chemical reaction
70
how many total amino acids are needed for the human body to produce all the proteins needed
20 amino acids
71
what is the oxidation number of oxygen
-2
72
general formula of a carbohydrate
(CH2O)n
73
what does ph measure
the concentration of hydrogen ions
74
which of the following is emitted during beta decay
electron
75
isotope
Atoms with the same number of protons and electrons but different neutrons
76
why does increasing the surface area of reactants or catalyst increase the rate of a reaction
it increases the likelihood of molecules encountering one another
77
elements in the modern periodic table are arranged by increasing what
atomic number
