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Science-9th Grade > Chemistry > Flashcards

Chemistry Flashcards

1
Q

PTOM: All matter is made up of

A

Tiny Particles

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2
Q

PTOM: All particles of _______ are the _____ Different ____ are made up of different ______

A

One substance, same, substances, particles

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3
Q

PTOM: Paticles are always

A

Moving

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4
Q

PTOM: Particles move _____ at ___ compared to ___ temperatures.

A

Faster, high, low.

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5
Q

PTOM: Particles are ____ to one another these forces are stronger when particles are _______

A

attracted, closer together

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6
Q

Describe Particles in a solid

A

Particles are very close. Strong attraction. Vibration only back and forth.

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7
Q

Describe particles in a liquid

A

Particles are close. Attraction. Particles can slide past each other.

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8
Q

Describe particles in a gas

A

Particles are very far apart. Particles are moving rapidly.

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9
Q

Explain the breakdown of matter

A

Matter
Pure Substances Mixtures
Element Compound Homo.
Hetero

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10
Q

Matter is: Anything that has _______ and _________ (has ________). Matter can be classified into __________ and ________

A

mass, takes up space, volume, pure substances, mixtures

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11
Q

A Pure substance: substances made up of only _______ of _______ or ________

A

one type, atom, molecules

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12
Q

Mixtures contain

A

two or more substances

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13
Q

Elements contain ___________–_ found on the

A

one element, periodic table

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14
Q

Compounds contain ___________ element in a fixed ratio

A

more than 1

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15
Q

Homogeneous mixtures are a substance that appears the _____________ aka solution

A

same throughout

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16
Q

Heterogeneous mixtures are a substance where the material is __________ (parts can be seen) mechanical mixtures

A

not uniform

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17
Q

Physical Property (Qualitative), Examples

A

Can be observed by your 5 senses. State colour odour mass volume stregnth flexibility malleability, lustre

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18
Q

Physical property (Quantitative) Examples

A

Can be measured. Mass or weight, volume temperature melting point, density

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19
Q

Chemical properties, examples

A

Describes how a substance changes to form one or two new substances. Combustibility, reactivity (with water, acids oxygen), flammability, acidity or basicity, toxicity, radio activity

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20
Q

Physical change definition. Examples

A

Involves a tranformation in the form of a substance and is reversible. This would include dissolving or any change of state, such as melting condensation or freezing. Chopping wood, melting ice and boiling water.

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21
Q

Chemical change, examples

A

Involves a transformation in the chemical structure or make-up of the matter involved. It is NOT reversible and always involves the formation of a new substance. burning wood, souring milk, cookin an egg, baking a cake, rusting of iron, digesting food.

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22
Q

What are the 5 indication of a chemical change

A

Colour change, formation of a solid (percipitate), production of an odour, temperature change, or formation of bubbles.

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23
Q

What is an atom

A

The smallest part of a chemical element is an atom.
The word atom comes from the Greek word atomos meaning indivisble.
With new discoveries and prgressive scientific experiments, the concept of an atom has changed overtime.
Atomic theory is the study of the nature of atoms and how they combine to form all types of matter.
An understanding of atoms and their structure can help us predict many of the properties of matter.

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24
Q

Protons

A

p+
Positive charge
1 amu (atomic mass unity)
located in the nucleus

25
Neutrons
n0 Neutral 1 amu Neuclues location
26
Electrons
e- Negative 1/1837 amu Orbit/shell/ring
27
The periodic table 2 points
The periodic table is organized by Periodic law The chemical and physical properties of the elements recur periodically when the elements are arranged and organized in order of increasing atomic number
28
Rows = Columns=
Period Group
29
Dmirtir Medeleeve How his worked Problems
HHW: Put elements in rows by increasing atomic weight put elements in columns by the way they reacted P: He left blank spaces for undiscovered elements He broke the pattern of increasing atomic weight to keep similar reating elements together
30
Our version of the PT 3 points
Now elements are put into rows by increasing atomic number, each box represents an element. The abbreviation shown in the box for each element is called its atomic symbol
31
Locations Metal Nonmetals Metalloids
Left & Middle Right Staircase
32
Physical properties of metal
Malleable, ductile, lustrous, good conductors of heat and electricity. Solid (liquid mercury)
33
Physical properties of non metals
Brittle, not ductile, dull, poor conductors of heat and electirciy, cand be solid or gasses and bomine is a liquid
34
How to draw Bohr Rutherford
1. Determine number of protns neutrons and electons, 2. Place protons and neutrons in the nucleus 3. Draw shells around nucleus 4. Fill shells with 2,8,8,2 pattern
35
How to draw Lewis-Dot diagrams
1. Write the element symbol 2. Determine the number of valence electrons (group #) 3. Draw the valence electrons aroound the symbol
36
Group 1: Alkalai Metals Properties
Very reactive always combined with something else in nature. Highly reactive to air and water. Soft enought to cut with a knife Lustrous silver in colour Low density
37
Group 2 Alkaline Earth Metals Properties
Reactive metals that are always combined with non-metals in nature, not as reactive as group 1. Reactive in hot water Burn Brightly Hard, shiny and silvery Serveral are important mineral nutrients
38
Group 3-12: Transition metals properties
Number of valece electrons varies, less reactive harder metals Metals used as "metals" strong, non-toxic
39
Staircase: Metalloids properties
Have properties of metals and non-metals Britlle, Lustrous Semi conductors used in computers
40
Groups 13-16: Other Non-Metals Properties
Cannot conduct electricty or heat well Very brittle Do not reflect light
41
Group 17: Halogens properties
Very reactive & volatile Diatomic (in pairs) Alwaus combined with other elements in nature Used as disinfectants All states present
42
Group 18: Noble gassses properties
Full valence shellVery unreactive monatomic gases Colourless tasteless odourless Used in neon signs Glow bright if electrical current is passed through
43
Atoms being put together
Atoms chemically joined with other to form molecules Chemical is the notation used to indicate the type and number of atoms in a pure substance.
44
Counting atoms Water
Formula: H20 Atoms Hydrogen Oxygen 2 hydro 1O
45
Most elements are
monatomic
46
Seven elements are ____ what are they
Diatomic, Hydrogen, Nitrogen, Oxygen, florine, clorine, bromine, iodine
47
Counting atoms how to do
Symbol represents 1 element Subscript after the number represents more than one of the previous element Brackets mean (P2K1)3 = 6P 3 K Coefficient means 3 of that formula = 3H20=6H 3O
48
Chemical Bonding: Why do they? How?
To become stable, and get a full valence shell By a metal donating electrons to non-metal (ionic) 2 non-metals sharing (covalent)
49
Ionic bonding:
Ionic compoundsmetal loses electrons non-metal gains completing valence shells. Elements in same family develop same ionic charges, metals tend to lose electrons (cations), and non metals gain (anions)
50
Ion formation
If electron is lost it becoms pawsitive (cation) gains (negative anion) oppisitely charged ions attract eachother and form ionic compounds
51
Molecular compuounds
occur when two or more non-metals share their electrons to complete their valence shells
52
naming binary ionic compounds
state name of the metal (cation) State the name of the non-metal (anion) change ending to ide
53
Writing formulas for bonds
Write symbols starte with metal, write ionic charge (no - or +) criss-cross the charges, reduce to lowest terms
54
Covalent bonding
Share electrons to fill valence shell Caused by two non-metals bonding When writing formulas same as ionic Naming adding prefixes
55
Covalent bond naming
State the name of the first element If there is more than 1 add the prefix State the name of the second element, add prefix
56
examples of acids, solvents, glues why they are dangerous
Acid: Rust Remover is corrosive and toxic Glues: glue is toxic, dangerous if ingested Solvent: acetone health problems toxic
57
Examples of paints and stains and why they are dangerous
Indoor Paint, Outdoor stain Breathing solvent paint fumes for too long can cause headaches, dizziness, and nausea.
58
Examples of aerosols & why dangerous
Lysol OFF Exposure to aerosols can lead to short-term acute symptoms, like asthma and bronchitis, and long-term chronic irritation and inflammation of the respiratory track, which can potentially lead to cancer.
59
All categories of dangerous household waste halton
Acids, solvents, glues Paints and stains Aerosols Pesticides, garden chemicals fertilizers Automotive liquids, oil filters Sharps Batteries Mercury-containing devices Pressurized cylinders (less than 20 lbs) Fluorescent lights, CFL bulbs Personal care products Medications (prescription and over-the-counter) Household cleaners, bleach, pool chemicals Waste cooking oil

Science-9th Grade (4 decks)

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