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Science-9th Grade > Chemistry > Flashcards

Chemistry Flashcards

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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
Q

Neutrons

A

n0
Neutral
1 amu
Neuclues location

26
Q

Electrons

A

e-
Negative
1/1837 amu
Orbit/shell/ring

27
Q

The periodic table
2 points

A

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
Q

Rows =
Columns=

A

Period
Group

29
Q

Dmirtir Medeleeve
How his worked
Problems

A

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
Q

Our version of the PT
3 points

A

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
Q

Locations
Metal
Nonmetals
Metalloids

A

Left & Middle
Right
Staircase

32
Q

Physical properties of metal

A

Malleable, ductile, lustrous, good conductors of heat and electricity. Solid (liquid mercury)

33
Q

Physical properties of non metals

A

Brittle, not ductile, dull, poor conductors of heat and electirciy, cand be solid or gasses and bomine is a liquid

34
Q

How to draw Bohr Rutherford

A
  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
Q

How to draw Lewis-Dot diagrams

A
  1. Write the element symbol
  2. Determine the number of valence electrons (group #)
  3. Draw the valence electrons aroound the symbol
36
Q

Group 1: Alkalai Metals Properties

A

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
Q

Group 2 Alkaline Earth Metals Properties

A

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
Q

Group 3-12: Transition metals properties

A

Number of valece electrons varies, less reactive harder metals
Metals used as “metals” strong, non-toxic

39
Q

Staircase: Metalloids properties

A

Have properties of metals and non-metals
Britlle,
Lustrous
Semi conductors used in computers

40
Q

Groups 13-16: Other Non-Metals Properties

A

Cannot conduct electricty or heat well
Very brittle
Do not reflect light

41
Q

Group 17: Halogens properties

A

Very reactive & volatile
Diatomic (in pairs)
Alwaus combined with other elements in nature
Used as disinfectants
All states present

42
Q

Group 18: Noble gassses properties

A

Full valence shellVery unreactive monatomic gases
Colourless tasteless odourless
Used in neon signs
Glow bright if electrical current is passed through

43
Q

Atoms being put together

A

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
Q

Counting atoms Water

A

Formula:
H20
Atoms Hydrogen Oxygen
2 hydro 1O

45
Q

Most elements are

A

monatomic

46
Q

Seven elements are ____ what are they

A

Diatomic, Hydrogen, Nitrogen, Oxygen, florine, clorine, bromine, iodine

47
Q

Counting atoms how to do

A

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
Q

Chemical Bonding:
Why do they?
How?

A

To become stable, and get a full valence shell

By a metal donating electrons to non-metal (ionic)
2 non-metals sharing (covalent)

49
Q

Ionic bonding:

A

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
Q

Ion formation

A

If electron is lost it becoms pawsitive (cation)
gains (negative anion)
oppisitely charged ions attract eachother and form ionic compounds

51
Q

Molecular compuounds

A

occur when two or more non-metals share their electrons to complete their valence shells

52
Q

naming binary ionic compounds

A

state name of the metal (cation)
State the name of the non-metal (anion) change ending to ide

53
Q

Writing formulas for bonds

A

Write symbols starte with metal, write ionic charge (no - or +) criss-cross the charges, reduce to lowest terms

54
Q

Covalent bonding

A

Share electrons to fill valence shell
Caused by two non-metals bonding
When writing formulas same as ionic
Naming adding prefixes

55
Q

Covalent bond naming

A

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
Q

examples of acids, solvents, glues why they are dangerous

A

Acid: Rust Remover is corrosive and toxic
Glues: glue is toxic, dangerous if ingested
Solvent: acetone health problems toxic

57
Q

Examples of paints and stains and why they are dangerous

A

Indoor Paint, Outdoor stain
Breathing solvent paint fumes for too long can cause headaches, dizziness, and nausea.

58
Q

Examples of aerosols & why dangerous

A

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
Q

All categories of dangerous household waste halton

A

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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