nine

Note : flashcards are all heavily squished & simplified . I reccomend making ur own

[scienceenine]

— NINE

science mindmaps turned into flashcards .

some bits may be wrong, inaccurate, or missing something . Mb

make ur own if these SUCK which they do . Trust me

Main website - click here !

[scienceenine]

P2 (split into 6 flashcards)

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Front:

Definitions (heating).

Back:

Conductor: Allows heat energy to flow.

Insulator: Prevents heat energy escaping.

Dissipated: Spread out and lost energy.

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Front:

Difference between heat and temperature & thermal conductivity meaning

Back:

Heat: Energy being transferred.

Temperature: How hot something already is.

High thermal conductivity: Faster heat transfer.

Low thermal conductivity: Slower heat transfer.

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Front:

What is specific heat capacity?

Back:

Energy needed to heat 1 kg of a substance by 1°C.

High SHC = needs more energy to warm up.

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Front:

SHC equation + symbols.

Back:

𝐸 = 𝑚 𝑐 Δθ — (θ could also be shown as an 𝑇)

E: energy (J)

m: mass (kg)

c: SHC (J/kg°C)

ΔT: temperature change (°C)

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Front:

The three heat‑transfer processes

Back:

Conduction: Heat moves through touching particles

Convection: Warm fluids rise, cool fluids sink

Radiation: Heat travels by waves; no particles needed

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Front:

Convection currents + infrared radiation basics.

Back:

Hot particles spread out, become less dense, rise; cool particles sink.

All objects emit and absorb IR.

Hotter objects emit more radiation.

Black bodies: perfect absorbers and emitters.

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[scienceenine]

B2 (split into 2 flashcards)

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Front:

Stem cells: types, potentials, and key terms

Back:

• Specialised cell: adapted for a specific function

• Differentiation: unspecialised → specialised

• Pluripotent: can become any cell type (embryonic stem cells, meristems in plants)

• Multipotent: limited to related cell types (adult stem cells in bone marrow)

• Embryonic stem cells: pluripotent, undifferentiated, from early embryo

• Adult stem cells: multipotent, found in bone marrow

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Front:

Advantages and disadvantages of embryonic stem cells

Back:

Advantages:

• Can cure medical conditions

• Would otherwise be discarded from research

• Can form any cell/tissue type

• Useful for research

• Could reduce organ transplant waiting times

Disadvantages:

• Ethical concerns (potential life destroyed, religious issues)

• Risk of viral transmission or infection

• Shortage of donors/eggs

• Egg collection has risks

• Low success rate

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Front:

Mitosis, meiosis, and the cell cycle

Back:

• Meiosis: produces gametes (sperm/egg)

• Mitosis: cell growth; organelles duplicate; produces 2 genetically identical daughter cells

• Mitosis steps:

1. Chromosomes replicate

2. Chromosomes line up

3. Spindle fibres pull copies apart

4. Nucleus reforms

5. Cytoplasm divides

• Cell cycle:

1. Replication

2. Mitosis

3. Cytokinesis

[scienceenine]

B1 (split into 3 flashcards)

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Front:

Diffusion, osmosis, and active transport

Back:

• Diffusion: particles move high → low concentration

• Osmosis: water moves from dilute → concentrated through a partially permeable membrane

• Active transport: moves substances low → high concentration using energy

• Rate factors: distance + surface area + gradient (gradient doesn’t help active transport)

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Front:

Eukaryotic vs prokaryotic + plant cell parts

Back:

• Eukaryotic: has nucleus (animal + plant cells)

• Prokaryotic: no nucleus, loops of DNA (bacteria)

• Plant cell organelles: nucleus, chloroplasts, cytoplasm, ribosomes, cell wall, cell membrane, permanent vacuole

• Yellow‑labelled = not in animal cells

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Front:

Microscopes and magnification

Back:

• Light microscope: beam of light, cheap, portable, views living tissue

• Electron microscope: beam of electrons, higher resolution, cannot view living tissue, expensive

• Magnification: eyepiece × objective OR image size ÷ real size

• Resolution: ability to distinguish separate objects

[scienceenine]

P1 (Split into 2 flashcards) click here to go back

Front:

Energy definitions, conservation & key energy formulas

Back:

Wasted energy: dissipated, usually as thermal

Useful energy: energy you want

Closed system: no energy enters or leaves

Conservation of energy: energy cannot be created or destroyed

Kinetic energy: Ek = 0.5 k m v2

Elastic potential = Ek = 0.5 k e2

GPE: Ep = m g h

Work done: Force × Distance

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Front:

Energy stores and pathways

Back:

8 stores:

kinetic

thermal

GPE

chemical

nuclear

electrostatic

elastic

magnetic

4 pathways:

forces

electric current

waves

heating

[scienceenine]

C2 (Split into 3 flashcards) click here to go back

Front:

Reactivity trends in Groups 1, 7, and 0

Back:

Group 1: Reactivity increases going down (outer electron farther, easier to lose)

Group 7: Reactivity decreases going down (harder to gain an electron)

Group 0: Unreactive because full, stable outer shells

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Front:

Halides, alkali metals, and displacement reactions

Back:

Halide: Metal + Halogen → Metal halide

Alkali + Water: → Alkali hydroxide + Hydrogen

Displacement: More reactive halogen replaces a less reactive one

Inert: Means unreactive and stable

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Front:

Newland vs. Mendeleev + Group 1/7/0 properties

Back:

Newland (1864): Ordered by mass; saw repeating patterns; forced wrong groupings

Mendeleev (1869): Left gaps; accurate predictions; broke mass order for properties

Group 1: Low density, shiny, soft metals, good conductors

Group 7: Coloured, toxic non‑metals, poor conductors

Group 0: Colourless gases, very unreactive, poor conductors

[scienceenine]

C1 (Split into 3 flashcards) click here to go back

Front:

Key definitions in atomic structure

Back:

• Atom: smallest particle of matter, not visible to the naked eye

• Element: made of only one type of atom

• Compound: two or more elements chemically bonded

• Isotopes: same element, different number of neutrons

• Ions: atoms with a charge from gaining/losing electrons

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Front:

Subatomic particles + electron shells

Back:

Reactivity depends on electrons, not isotopes

Law of conservation of mass: atoms aren’t created or destroyed in reactions

Protons: mass 1, charge +1

Neutrons: mass 1, charge 0

Electrons: mass ~0, charge –1

Shell rule:

1st shell: 2 electrons

2nd shell: 8 electrons

3rd shell: 8 electrons

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Front:

Timeline of atomic model development

Back:

Democritus (400 BCE): matter made of tiny particles

Dalton (1803): atoms are solid spheres

Thomson (1897): electrons discovered; plum pudding model

Rutherford (1911): nucleus + empty space

Bohr (1913): electrons in fixed orbits

Schrödinger (1926): electron clouds

Chadwick (1932): neutrons discovered